The slowest step of a reaction mechanism is called the
A.) Elementary Step
B.) Inhibitor
C.) Rate Law
D.) Rate-Determining Step

Answer:in decreasing pattern; AlN>CaO>LiCl>KI.

Explanation:

The energy required to break apart an ionic solid and convert its component atoms into gaseous ions is known as the LATTICE ENERGY.

LATTICE ENERGY has a trend on the periodic table. The trend shows the relationship between LATTICE ENERGY AND THE ATOMIC RADIUS.

Lattice energy is related to solubility, volatilty and hardness.

Down the group on the periodic chart, the ATOMIC RADIUS INCREASES, THE LATTICE ENERGY DECREASES. Which means that between Lithium ion and potassium ion, Lithium ion will have higher lattice energy than that of potassium.

The trend ACROSS THE PERIOD is that, as we go across the period, the charges on metals increase,consequently INCRESING THE LATTICE ENERGY. Between Aluminum ion with a positive charge of three and Calcium with a positive charge of two, Aluminium ion has higher charge, which means it has more lattice energy than calcium.

The ionic compounds in order of their decreasing amount of energy are AIN>CaO>LiCl>Kl.

The lattice energy is used for the estimation of the strength of the bond that is in ionic compounds.

It should be noted that the higher the charge of the ion, the higher will be the lattice energy. On the other hand, the smaller the radius of ion, the larger will be the lattice energy.

Therefore, the ionic compounds in order of their decreasing amount of energy will be AIN>CaO>LiCl>Kl.

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Answer:

Energy change associated with the gaining of an electron by the atom in the gaseous state.

Explanation:

What is electron affinity?

The change in enthalpy, entropy, and free energy were calculated for the dehydrogenation reaction of ethylbenzene into styrene. The reaction was found to be endothermic and results in a decrease in overall disorder. Under the given conditions, the reaction will never be spontaneous.

The processes involved in the production of styrene from ethylbenzene are fairly complex and require knowledge of thermodynamics. We'll begin with ΔH°rxn, which is found by subtracting the enthalpy (ΔH) of the reactants from that of the products: ΔH°rxn = [ΔH°f(styrene)] - [ΔH°f(ethylbenzene)] = 103.8 kJ/mol - (-12.5 kJ/mol) = 116.3 kJ/mol. This means the reaction is endothermic, as heat is absorbed.

The change in entropy ΔS°rxn, obtained likewise, is [S°(styrene) - S°(ethylbenzene)] = (238 J/mol·K - 255 J/mol·K) = -17 J/mol·K. This indicates a decrease in disorder in the system.

With these, we can calculate the change in free energy ΔG°rxn at a given temperature (T) using the equation ΔG°rxn = ΔH°rxn - TΔS°rxn. Substituting the known values at 298 K, ΔG°rxn = 116.3 kJ/mol - (298 K)(-17 J/mol·K) = 121.2 kJ/mol, indicating a non-spontaneous reaction.

For the reaction to be spontaneous, ΔG°rxn must be less than zero. Solving for T in the above equation with ΔG°rxn = 0, yields T = ΔH°rxn / ΔS°rxn = 116.3 kJ/mol / -17 J/mol·K ≈ -6840 K. This value is negative, implying the reaction is never spontaneous under the given conditions.

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Answer: The nitrogen atom is getting reduced.

Explanation:

Oxidation reaction is defined as the reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

[tex]X\rightarrow X^{n+}+ne^-[/tex]

Reduction reaction is defined as the reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

[tex]X^{n+}+ne^-\rightarrow X[/tex]

The given chemical equation follows:

[tex]Fe_2S_3+12HNO_3\rightarrow 2Fe(NO_3)_3+3S+6NO_2+6H_2O[/tex]

On reactant side:

Oxidation state of iron atom = +3

Oxidation state of nitrogen atom = +5

Oxidation state of sulfur atom = -2

On product side:

Oxidation state of iron atom = +3

Oxidation state of sulfur atom = 0

Oxidation state of nitrogen atom in [tex]NO_2[/tex] = +4

Oxidation state of nitrogen atom in [tex]Fe(NO_3)_3[/tex] = +5

As, the oxidation state of nitrogen atom in [tex]NO_2[/tex] is decreasing from +5 to +4. So, it is getting reduced.

And, oxidation state of sulfur atom is increasing from -2 to 0. So, it is getting oxidized.

Hence, the nitrogen atom is getting reduced.

The element that gets reduced in the chemical reaction is nitrogen.

Reduction in chemistry means when an atom accepts electrons to become more negatively charged.

According to this question, the following chemical reaction is given:

Fe2S3 + 12HNO3 → 2Fe(NO3)3 + 3S + 6NO2 + 6H2O

On reactant side:

On product side:

As indicated above, the oxidation number of nitrogen reduces from +5 to +4, hence, it is the element that gets reduced.

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The minimum standard reduction potential at the cathode in this galvanic cell should be at least 1.23V to provide the needed power. There is no defined maximum limit for this value. A suitable half-reaction for the cathode could involve the reduction of silver ions to silver metal.

For a galvanic cell to work, the potential at the cathode must be greater than that at the anode. In this specific case, the reduction potential at the anode, E0anode, is given as +0.13V. The difference in potentials between the cathode and anode corresponds to the provided voltage of the cell, which is 1.10V in this particular scenario.

Using this information, the reduction potential at the cathode can be calculated using E0cell = E0cathode - E0anode formula. Substituting the known values, 1.10V = E0cathode - (+0.13V), we find that E0cathode should be at least 1.23V to provide the necessary power.

There is technically no maximum limit for E0cathode as increasing this value only increases the power provided by the cell. As for a suitable half-reaction, a reduction of silver ions (Ag+) to silver metal (Ag) having a reduction potential of +0.80V could be used:

Ag+ + e- --> Ag

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There is a minimum standard reduction potential for the cathode: 0.97 V. The maximum standard reduction potential is generally assumed to be less than +2.87 V. An example of a balanced cathode half-reaction is 2H⁺ (aq) + 2e⁻ → H₂ (g).

Yes, there is a minimum standard reduction potential for the half-reaction at the cathode. The cell potential, E°cell, is calculated as:

Given that E°anode = -0.13 V (since it’s the reduction potential, but we use it as an oxidation potential here), and the cell must provide at least 1.10 V, we have:

Solve for E°cathode:

Yes, there is a maximum standard reduction potential. Practically, the maximum standard reduction potential of the cathode is determined by the potential of the reference electrode (often chosen to be +2.87 V for fluorine). Therefore, any standard reduction potential must be less than this value.

Answer: [tex]5.81\times 10^6J/mol[/tex]

Explanation:

Heat of combustion is the amount of heat released when 1 mole of the compound is completely burnt in the presence of oxygen.

[tex]C_{12}H_{22}O_{11}(s)+12O_2\rightarrow 12CO_2(g)+11H_2O(g)[/tex]

To calculate the moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{0.05392g}{342g/mol}=1.577\times 10^{-4}moles[/tex]

Thus [tex]1.577\times 10^{-4}moles[/tex] of sucrose releases =  916.6 J of heat

1 mole of sucrose releases =[tex]\frac{916.6}{1.577\times 10^{-4}}\times 1=5.81\times 10^6J[/tex] of heat

Thus ∆H value for the combustion reaction is [tex]5.81\times 10^6J/mol[/tex]

The ∆H for the combustion reaction of 0.05392 g of sucrose, given that the qrxn is -916.6 J, is calculated to be approximately -58364.2 kJ. This value is negative indicating an exothermic reaction where heat is released.

In this problem, we are tasked with finding the enthalpy change, or ∆H, for the combustion reaction of sucrose. The heat of the reaction, qrxn, is given as -916.6 J for a 0.05392 g pellet of sucrose.

Firstly, we have to convert the grams of sucrose to moles. The molecular weight of sucrose, C12H22O11, is about 342.3 g/mol so the moles of sucrose burned would be 0.05392 g ÷ 342.3 g/mol = 0.000157 mol.

Next, the change in enthalpy per mole of sucrose can be calculated using ∆H = qrxn / moles of sucrose which gives us -916.6 J / 0.000157 mol = -58364152.2293 J/mol. Since the question requires the answer in kJ, we must divide this by 1000 to convert J to kJ. Hence, ∆H = -58364.1523 kJ/mol.

It is important to note that ∆H is negative because the reaction is exothermic, meaning heat is released during the combustion of sucrose. Therefore, the ∆H for the combustion reaction of sucrose is approximately -58364.2 kJ.

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Answer:

False statement is

At a given temperature, for a given gas, every molecule has the same speed

Explanation:

While checking each and every statement given

The mean free of a molecule actually depends on the size of the molecule because the mean free path is defined as the average distance between two successive collisions of the gas molecules

If the size of the molecule is more, the average distance between two successive collisions decrease and as a result the mean free path of the molecule decreases

Dalton's law of partial pressures is applicable for only ideal gases which means we are assuming that the size of the molecule of a gas is negligible and there are no intermolecular forces of attraction

These two assumptions gets applied at high temperature and low pressure

So Dalton's law of partial pressures tells us that total pressure of the gas is equal to the sum of the partial pressures of the individual gas components

∴ It explains the independent nature of the gas molecule

At a given temperature, for a given gas, all molecules of the gas do not have same speed but overall the average speed of the gas remains same because speed of each molecule of a gas depends on the collision with other molecules of the gas and as the collisions can't be the same therefore molecules of a gas have different speeds

Actually pressure is generated by the collisions of molecules with the container walls because when the gas molecules collide with the container they generate a force which in turn produce the pressure

At high pressure gas do not tend to behave ideally as there will be intermolecular forces and we will write the ratio of PV/nRT as Z which is the compressibility factor of a gas and it will be different for different gases as different gases has different intermolecular forces of attraction

Answer:

The standard molar enthalpy of formation of 1 mole of NO gas is 90.25 kJ/mol.

Explanation:

We have :

[tex]N_2(g) + 2O_2 \rightarrow 2NO_2(g), \Delta H^o_{1} = 66.4 kJ[/tex]

[tex]2NO(g) + O_2\rightarrow 2NO_2(g),\Delta H^o_{2} = -114.1 kJ[/tex]

To calculate the standard molar enthalpy of formation

[tex]N_2+O_2\rightarrow 2NO(g),\Delta H^o_{3} = ?[/tex]...[3]

[1] - [2] = [3] (Hess's law)

[tex]N_2+O_2\rightarrow 2NO(g),\Delta H^o_{3} = ?[/tex]

[tex]\Delta H^o_{3} =\Delta H^o_{1} - \Delta H^o_{2} [/tex]

[tex]\Delta H^o_{3}=66.4 kJ - [ -114.1 kJ] = 180.5 kJ[/tex]

According to reaction [3], 1 mole of nitrogen gas and 1 mole of oxygen gas gives 2 mole of nitrogen monoxide.

So, the standard molar enthalpy of formation of 1 mole of NO gas :

[tex]\Delta H^o_{f,NO}=\frac{\Delta H^o_{3}}{2 mol}[/tex]

[tex]\Delta H^o_{f,NO}=\frac{180.5 kJ}{2 mol}=90.25 kJ/mol[/tex]

To calculate the standard molar enthalpy of formation of NO(g), the given reactions are used by reversing the second reaction and adding its enthalpy change to the first reaction's ΔH. Dividing the total by 2 gives 90.25 kJ/mol for the formation of 1 mole of NO(g) from its elements.

To calculate the standard molar enthalpy of formation of NO(g), we can use the given enthalpy changes for the reactions provided. The two reactions are:

We want to find the enthalpy change for the formation of NO(g) from its elements, which is N2(g) and O2(g). This is the standard molar enthalpy of formation for NO(g). We can set up an enthalpy diagram to help visualize the process.

Working through the math:
ΔHf[NO] = (66.4 kJ + 114.1 kJ) / 2
ΔHf[NO] = 180.5 kJ / 2
ΔHf[NO] = 90.25 kJ/mol

Therefore, the standard molar enthalpy of formation of NO(g) is 90.25 kJ/mol.

Answer:

Evaporate minerals are more soluble than calcite and quartz.

Explanation:

Evaporate minerals are the water soluble minerals which at higher concentration precipitate out and crystallized forming rocks.

example of chemicals present are:

chlorides and sulphates.

Quartz is silica (very less soluble, or insoluble)

Calcite is calcium carbonate, again an insoluble salt.

Thus

Evaporate minerals are more soluble than calcite and quartz.

Answer:

When the solution (with phenolphthalein) changes to colorless

Explanation:

When titrating with HCl is common to add phenolphthalein as an acid-base indicator.

Phenolphthalein is pink or fucsia when added into a basic solution. On the other hand when it is in acid solutions, is colorless.

So, when titrating, the NaOH solution will be initialy pink due to the phenolphthalein and when reaching the equivalence point, that color will fade out into colorless. This is how you know you hace reached the equivalent point.

The standard cell potential (E°cell) for the given electrochemical reaction is approximately +0.9 V. Here option C is correct.

Identifying the Redox Reactions and Potentials

The given balanced equation reveals two processes: an oxidation and a reduction.

Oxidation: [tex]Sn$^{2+}$[/tex] loses two electrons to become [tex]Sn$^{4+}$[/tex]. This can be represented as:

[tex]$$Sn^{2+}(aq) \rightarrow Sn^{4+}(aq) + 2e^-$$[/tex]

Reduction: [tex]Fe$^{3+}$[/tex] gains one electron to become [tex]Fe$^{2+}$[/tex]. This can be represented as:

[tex]$$Fe^{3+}(aq) + e^- \rightarrow Fe^{2+}(aq)$$[/tex]

Next, we need to find the standard reduction potentials (E°) for these half-reactions. Remember, we need the reverse of the oxidation reaction, so look for the potential of:

[tex]$$Sn^{4+}(aq) + 2e^- \rightarrow Sn^{2+}(aq)$$[/tex]

From the provided table, find the value for this and the given reduction reaction:

Oxidation: E° = -0.154 V

Reduction: E° = +0.771 V

Calculating the Cell Potential (E°cell)

The reduction occurs at the cathode (positive) and the oxidation at the anode (negative). Therefore, the cell potential is calculated by:

[tex]$$E^{\circ}_{cell} = E^{\circ}(\text{cathode}) - E^{\circ}(\text{anode})$$[/tex]

Substituting the values:

[tex]$$E^{\circ}_{cell} = (+0.771 \text{ V}) - (-0.154 \text{ V})$$[/tex]

[tex]$$E^{\circ}_{cell} \approx +0.925 \text{ V}$$[/tex]

However, the answer choices only have one decimal place, so we need to round: [tex]$$E^{\circ}_{cell} \approx \boxed{+0.9 \text{ V}}$$[/tex]. Here option C is correct.

Complete question:

The standard cell potential (E°cell) for the voltaic cell based on the reaction below is ________.

Sn2+(aq) + 2Fe3+(aq) --> 2Fe2+(aq) + Sn4+(aq)

Half-reaction E°(V)

Cr3+(aq) + 3e - --> Cr(s) - 0.74

Fe2+ (aq) + 2e - --> Fe(s) - 0.440

Fe3+(aq) + e - --> Fe2+(s) + 0.771

Sn4+(aq) + 2e - --> Sn2(aq) + 0.154

a) +0.46 V

b) +0.617 V

c) +0.9 V

d) -0.46 V

e) +1.21 V

Final answer:

To run out of oxygen and acetylene at the same time, the acetylene tank should be filled to a pressure of 62.14 atm.

Explanation:

To ensure that you run out of oxygen and acetylene at the same time, the number of moles of oxygen and acetylene consumed must be equal. The volume ratio of oxygen and acetylene gases is 7.00 L : 3.00 L, which simplifies to 7 : 3. Therefore, the pressure ratio of oxygen to acetylene should also be 7 : 3. Given that the oxygen tank is filled to a pressure of 145 atm, the acetylene tank should be filled to a pressure of (145 atm) x (3/7) = 62.14 atm.

Answer:

Strong electrolyte

Explanation:

Bulb doesn't light when water is used because water doesn't have any appreciable amount of ions for the conduction of electricity.

Strong electrolytes ionize almost completely in solution, thus providing a huge amount of ions to conduct electricity. More the number of ions, more charge is carried and hence greater current and thus leading to bulb glowing brighter.

Weak electrolytes ionize partially in solution, thus providing some amount of ions for carrying charge. This results in a small amount of current going to the bulb and hence the bulb lights up with very low intensity.

Non electrolytes doesn't ionize either and hence is similar to water. These have almost zero conductivity and hence the bulb doesn't light at all.

Answer:

1. False

2. False

3. True

4. False

5. False

6. False

Explanation:

1. Because HNO₃ is corrosive when handling it is important to use gloves and also protection glasses. If it touches the skin, then it's important to wash the area affected.

2. The dilute of acid is exothermic, so it releases a huge amount of heat. For precaution, the acid must be added at the water slowly stirring, so it can be controlled.

3. Fe(NO₃)₃ is an oxidizer and in contact with the skin it can cause irritation, so it must be handled carefully and with protection.

4. KSC can irritate the eyes, so it's toxic.

5. KSCN is not inflammable and it's not combustible, so when heated it will only change the state for gas, but it will not cause the evolution of cyanide gas.

6. If KSCN reacts with a strong base, it will dissociate, and the ions SCN⁻, which can't react with the OH⁻ ions of the base. So, it will only cause the evolution of cyanide gas if it reacts with a strong acid.

The answers have been given according to which is True or False. It explores the science of chemicals, especially Nitric Acid.

What is a Chemical Reaction?

Two substances will achieve a reaction has occurs when the molecular or ionic structure of a substance is rearranged to create a new form.

The statements thus are:

1) True.

2) False.

3) True.

4) False

5) False

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The molecule acetonitrile or CH3CN, indeed has 16 valence electrons and a triple bond follows its Lewis structure. However, the statement that acetonitrile has a pair of nonbonding electrons is incorrect because all 16 valence electrons are used in the molecule's bonds.

The molecule in question is acetonitrile, or CH3CN. To analyze these statements, it's crucial to consider the Lewis structure of this molecule: the carbon atom bonded to three hydrogen atoms, that carbon bonded to another carbon atom, and that second carbon bonded to a nitrogen through a triple bond. Hydrogen has 1 valence electron, carbon has 4, and nitrogen has 5.

a. The combined total of valence electrons for acetonitrile is indeed 16 - (3x1 for hydrogen, 2x4 for carbon, and 1x5 for nitrogen).
b. There is a triple bond between the carbon and nitrogen atoms.
c. The entirety of the 16 valence electrons are used in the molecule's bonds, leaving no nonbonding electrons. This statement is false.
d. All atoms in the structure satisfy the octet rule, each having a complete outermost shell.
e. Neither carbon atom nor the nitrogen atom has a nonzero formal charge; all atoms in acetonitrile have a formal charge of zero.

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The false statement about acetonitrile (CH3CN) is that it has one pair of nonbonding electrons. All the outer shell electrons in acetonitrile are involved in bonding, hence, there are no non-bonding electrons in the molecule.

Based on your question about acetonitrile (CH3CN), which is an important industrial chemical, the statement that is FALSE is: Acetonitrile has one pair of nonbonding electrons. When drawing the Lewis structure for acetonitrile, we find that all the outer shell electrons are involved in bonding, hence, there are no non-bonding electrons in acetonitrile. The molecule's other properties mentioned in the options are correct: it has 16 valence electrons, a triple bond between the carbon and nitrogen atoms, all atoms satisfy the octet rule, and the carbon attached to the nitrogen, as well as the nitrogen atom itself, have nonzero formal charges due to the triple bond and unequal sharing of electrons.

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Answer:

[R] = [Z] > Q

Explanation:

Given the equilibrium:

                        X(g) + 2 Q(g) ⇄  R(g) + Z(g)

The equilibrium constant will be given by:

Kc = 1.3 x 105 at 50ºC =  [R] x [Z] / ( [X] x [Q]² )

This value is telling us that at equilibrium the products quantities will be much higher than the reactants.

Looking at the answer choices we see that (a) is false since this is an equilibrium not a areaction that goes to completion;(b) is is false because again this is an equilibrium and it would also imply that Kc is one; (c) is false because in the reaction the ratio is 1X : 2Q.

The last choice is the true statement since the equilibrium constant favors the products. This statement would haven true if Kc had been much less than one.

The concentration of the products are greater than the concentration of the reactants.

The correct answer to the question is [R] = [Z] > Q

Equilibrium constant, K is simply defined as the ratio of the concentration of the products raised to their coefficients to the concentration of the reactants raised to their coefficients.

We can write the equilibrium constant for the reaction as follow:

X(g) + 2Q(g) ⇄  R(g) + Z(g)

K = [R][Z] / [X] [Q]²

From the question given above, we were told that the equilibrium constant has a value of 1.3×10⁵ i.e

K = [R][Z] / [X] [Q]²

1.3×10⁵ = [R][Z] / [X] [Q]²

From the above, we can see that the equilibrium constant has a higher value. This simply means that the concentration of the products is greater than the concentration of the reactants at equilibrium.

Thus, correct answer to the question is:

[R] = [Z] > Q

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Answer:

The reaction will be spontaneous

Explanation:

To determine if the reaction will be spontaneous or not at this temperature, we need to calculate the Gibbs's energy using the following formula:

[tex]\Delta G= \Delta H - T * \Delta S [/tex]

If the Gibbs's energy is negative, the reaction will be spontaneous, but if it's positive it will not.

Calculating the [tex]\Delta G= -1267 - 473 K* \Delta S [/tex] :

[tex]\Delta G= -1267 - 473 K* \Delta S [/tex]

Now, other factor we need to determine is the sign of the S variation. When talking about gases, the more moles you have in your system the more enthropic it is.

In this reaction you go from 7 moles to 8 moles of gas, so you can say that you are going from one enthropy to another higher than the first one. This results in: [tex]\Delta S>0[/tex}

Back to this expression:

[tex]\Delta G= -1267 - 473 K* \Delta S [/tex]

If the variation of S is positive, the Gibbs's energy will be negative always and the reaction will be spontaneous.

Answer:

molarity of I3^-(aq) in the solution = 0.21 M

Explanation:

We are given the balanced chemical reaction and the volume and molarity of the  Na₂S₂O₃ so we can calculate the moles of the thiosulfate that were required, and then can calculate the molarity the  I₃⁻ by the definition of molarity.

First lets  convert the volume of Na₂S₂O₃ to liters:

35.8 mL x 1 L/1000 mL = 0.0358 L

# moles Na₂S₂O₃ = 0.350 mol/L x 0.0358 L = 0.0125 mol

From the stoichiometry of the reaction we know 2 mol Na₂S₂O₃ s react with 1 mol I₃⁻ , therefore mol of I₃⁻  will be given by

1 mol I₃⁻ / 2 mol Na₂S₂O₃  x 0.0125 mol Na₂S₂O₃ = 0.0063 mol  I₃⁻

and its molarity is:

0.0063 mol  I₃⁻ / 0.030 L = 0.21 M

Answer:

The order of solubility is AgBr <   Ag₂CO₃ < AgCl

Explanation:

The solubility constant give us the molar solubilty of ionic compounds. In general for a compound AB the ksp will be given by:

Ksp = (A) (B) where A and B are the molar solubilities = s²  (for compounds with 1:1  ratio).

It follows then  that the higher the value of Ksp the greater solubilty of the compound if we are comparing compounds with the same ionic ratios:

Comparing AgBr: Ksp = 5.4 x 10⁻¹³ with AgCl: Ksp = 1.8 x 10⁻¹⁰, AgCl will be more soluble.

Comparing Ag2CO3: Ksp = 8.0 x 10⁻¹²  with AgCl Ksp = AgCl: Ksp = 1.8 x 10⁻¹⁰ we have the complication of  the ratio of ions 2:1 in Ag2CO3,  so the answer is not obvious. But since we know that

Ag2CO3 ⇄ 2 Ag⁺ + CO₃²₋

Ksp Ag2CO3  = 2s x s = 2 s² =  8.0 x 10-12

s = 4 x 10⁻12 ∴ s= 2 x 10⁻⁶

And for AgCl

AgCl  ⇄ Ag⁺ + Cl⁻

Ksp = s² = 1.8 x 10⁻¹⁰  ∴ s = √ 1.8 x 10⁻¹⁰   = 1.3 x 10⁻⁵

Therefore, AgCl is more soluble than Ag₂CO₃

The order of solubility is AgBr <   Ag₂CO₃ < AgCl

Answer:

5.4 x 10^-13

Explanation:

Edmentum says it is correct

Answer: The value of [tex]K_c[/tex] is coming out to be 0.412

Explanation:

To calculate the number of moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]     .....(1)

Given mass of [tex]Sb_2S_3[/tex] = 1.00 kg = 1000 g   (Conversion factor: 1 kg = 1000 g)

Molar mass of [tex]Sb_2S_3[/tex] = 339.7 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of }Sb_2S_3=\frac{1000g}{339.7g/mol}=2.944mol[/tex]

Given mass of hydrogen gas = 10.0 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of hydrogen gas}=\frac{10.0g}{2g/mol}=5mol[/tex]

Given mass of hydrogen sulfide = 72.6 g

Molar mass of hydrogen sulfide = 34 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of hydrogen sulfide}=\frac{72.6g}{34g/mol}=2.135mol[/tex]

The chemical equation for the reaction of antimony sulfide and hydrogen gas follows:

                  [tex]Sb_2S_3(s)+3H_2(g)\rightarrow 2Sb(s)+3H_2S(g)[/tex]

Initial:            2.944      5

At eqllm:      2.944-x     5-3x         2x        3x

We are given:

Equilibrium moles of hydrogen sulfide = 2.135 moles

Calculating for 'x', we get:

[tex]\Rightarrow 3x=2.135\\\\\Rightarrow x=\frac{2.135}{3}=0.712[/tex]

Equilibrium moles of hydrogen gas = (5 - 3x) = (5 - 3(0.712)) = 2.868 moles

Volume of the container = 25.0 L

Molarity of a solution is calculated by using the formula:

[tex]\text{Molarity}=\frac{\text{Moles}}{\text{Volume}}[/tex]

The expression of [tex]K_c[/tex] for above equation, we get:

[tex]K_c=\frac{[H_2S]^3}{[H_2]^3}[/tex]

The concentration of solids and liquids are not taken in the expression of equilibrium constant.

[tex]K_c=\frac{(\frac{2.135}{25})^3}{(\frac{2.868}{25})^3}\\\\K_c=0.412[/tex]

Hence, the value of [tex]K_c[/tex] is coming out to be 0.412

The estimated value of K for the reaction Sb2S3 (s) + 3 H2 (g) <--> 2 Sb (s) + 3 H2S (g) at 713K is approximately 1. This estimate is based on initial and equilibrium moles and concentrations of H2 and H2S.

The reaction is Sb2S3 (s) + 3 H2 (g) <--> 2 Sb (s) + 3 H2S (g). This type of equation is a chemical equilibrium reaction. Because Sb2S3 and Sb are solids, they are not included in the equilibrium constant expression. Only H2 (g) and H2S (g) are included. To solve the problem, the initial moles of H2 and H2S need to be calculated, and the moles of H2S at equilibrium can be found. After finding the moles, they can be converted into concentrations by dividing by the volume of the container (25.0 L).

Initially, we have 1.00 kg of Sb2S3, which is excess and doesn't appear in the equilibrium equation. So, it can be ignored. Similarly, for hydrogen, 10 g converts to approximately 5 moles. Since no H2S is present initially, let's denote its moles as 0. When the equilibrium is established we know that only 72.6g of H2S is present and that is approximately 3 moles. By stoichiometry, 1 mole of H2 will form 1 mole of H2S. Therefore, 3 moles of H2 have been used to form 3 moles of H2S. Subtracting the used quantity from the total, there is approximately 2 moles of H2 left. Plugging all these into the equilibrium equation, we get K = [H2S]^3 / [H2]^3 which is approximately equal to 1.

This process illustrates the concept of chemical equilibrium and how to calculate the equilibrium constant, K, for a reaction. It emphasizes the importance of stoichiometry, the mole concept, and concentration when dealing with equilibrium reactions.

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The complete question is here:

A 1.00 kg sample of Sb2S3 (s) and a 10.0 g sample of H2 (g) are allowed to react in 25.0L container at 713K. At equilibrium, 72.6 g H2S (g) is present? What is the value of K at 713K for the following reaction? The value of Kp?

Sb2S3 (s) + 3 H2 (g) <--> 2 Sb (s) + 3 H2S (g)

Answer:

A polar molecule may have one or more lone pairs.

A polar molecule has an uneven distribution of electron density.

Explanation:

A molecule in which the dipole bonds will not cancel is a polar molecule. It depends on the geometry of the molecule, and the direction of the dipole. So, to be polar, the molecule must have at least one polar bond. It may have nonpolar bonds, but the total dipole must be different from 0.

A polar bond is formed between elements that have large differents in electronegativities, such as chlorine and hydrogen. When an atom has a large electronegativity, it has lone pairs of electrons in a bond because it has a small size and a great number of electrons in the valence shell. So, a polar molecule may have on or more lone pairs.

Because of the lone pairs presented, and because of the dipole different from 0, it will be partial charges in the atoms, so a polar molecule has an uneven distribution of electrons density.

A polar molecule is a molecule that has opposite charges at both ends of the molecule.

The true statements about polar molecules are;

To say that a molecule is polar means that it has opposite charges at either end of the molecule.

These charges result from uneven distribution of electrons in the molecule. This uneven distribution of electrons in the molecule is also caused by the large difference in electronegativity between the bonding atoms. This electronegativity difference causes the electron density of the bond to draw closer one of bonding atoms thereby conferring a partial negative charge on that atom and a resulting partial positive charge on the other atom.

Many polar molecules have lone pairs on atoms in the molecule such as NH3, H2O, H2S, etc.

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Answer:

Answers are in the explanation

Explanation:

A bomb calorimeter is a constant volume calorimeter in which medition of change in temperature allows the medition of change in internal energy (ΔU) for chemical reactions or physical changes.

This ΔU can be converted in ΔH thus:

ΔH = ΔU + PV

That means that:

A bomb calorimeter is a piece of equipment designed to measure delta H

As there was said:

Reactions carried out in a bomb calorimeter occur at constant volume

To calculate the heat absorbed or released by a reaction carried out in a bomb calorimeter, we use the equation: q = C * delta T

Where C is the heat capacity of the calorimeter, delta T is the change in temperature and q is the heat produced in the chemical or physical process

I hope it helps!

A bomb calorimeter measures the change in internal energy (delta E) of reactions, which occur at constant volume. The heat absorbed or released is calculated using the formula q = C x delta T.

A bomb calorimeter is a piece of equipment designed to measure delta E, or the change in internal energy, for reactions. Reactions carried out in a bomb calorimeter occur at constant volume. The heat absorbed or released by a reaction in this calorimeter is calculated using the equation q = C x delta T, where 'q' is the heat, 'C' is the heat capacity of the calorimeter, and 'delta T' is the change in temperature.

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Answer:

D.) Products are weakly favored

Explanation:

For the reaction:

2SO₃ ⇄ O₂ + 2SO₂ + 198kJ/mol

The kc is defined as:

kc = [O₂] [SO₂]² / [SO₃]²

As the kc is 8,1:

8,1 [SO₃]² =  [O₂] [SO₂]²

The products are favored 8,1 times. This is a weakly favored because the usual kc are in the order of 1x10⁴. Thus, right answer is:

D.) Products are weakly favored

I hope it helps!

Final answer:

For the reaction 2SO3 → O2 + 2SO2 with an equilibrium constant Kc of 8.1 at 25 °C, the products are weakly favored since Kc is greater than 1 but much less than 10^3.  So the correct answer is D.

Explanation:

The equilibrium constant Kc indicates whether the reactants or products are favored in a chemical reaction at equilibrium. For the reaction 2SO3 → O2 + 2SO2, the equilibrium constant Kc is given as 8.1 at 25 °C. Since the value of Kc is greater than 1, this means that the reaction favors the formation of products over reactants. If the Kc value was less than 1, the reactants would be favored.

According to the table provided, values of Kc greater than 103 indicate a strong tendency for the reaction to favor the formation of products, suggesting a strongly favored product side for such large Kc values. In this case, with a Kc of 8.1, which is greater than 1 but significantly less than 103, the products are favored to a lesser extent. Therefore, we could conclude that the products are weakly favored, making option D the correct answer.

Answer:

U⁴⁺  

Explanation:

Fluorine stabilizes metals in higher oxidation states with high M:F ratios.

Hard acids prefer to bind to hard bases.

U⁴⁺ is the hardest acid in the list and F⁻ is a hard base, so an eight-coordinate complex of U⁴⁺ is the most stable.

The metal ion that can most adequately exist in the form of 8-coordinate complex would be:

d). U⁴⁺  

Thus, option d is the correct answer.

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Answer:

A(aq) + 1 e⁻ → A⁻(aq) at the cathode and B(aq) → B⁺(aq) + 1e⁻ at the anode.

Explanation:

In the anode occurs the oxidation, in which the reducing agent loses electrons, and its oxidation number increases.

B(aq) → B⁺(aq) + 1e⁻

In the cathode occurs the reduction, in which the oxidizing agent gains electrons, and its oxidation number decreases.

A(aq) + 1 e⁻ → A⁻(aq)

In a voltaic cell, the anode is where oxidation occurs, and the cathode is where reduction occurs. Electrons flow from the anode (negative electrode) to the cathode (positive electrode). The anode reaction is B(aq) → B+(aq) + 1e−, and the cathode reaction is A(aq) + 1e− → A−(aq).

In a voltaic (galvanic) cell, two half-reactions occur at separate electrodes.

Let's break down the given reactions:

Electrode Identification

In summary, electrons flow from the anode to the cathode through an external circuit, and a salt bridge maintains charge balance.

The question is already answered from one point of view but I'll add BeH2 has sp hybridization and H2O has sp3 hybridization getting a different structure type cause where the electron pairs are located around the central atom, that means that you will see the next structures from these molecules.

Answer:

Water (HoH) has

2

bonding electrons and 2 lone pairs. The placement of these electrons is going to be a tetrahedral electron-pair geometry. The HBeH molecule has 2 bonding electron pairs and 0 lone pairs. The bonding pairs must be as far from one another as possible.

Explanation:

I hope that helps any one in the future who needs it <3

The attraction between ions in a crystal depends on the size of the ions. Since chloride ion is smaller than bromide ion, the statement LiCl > LiBr is correct.

The attraction between oppositely charged ions in the crystal lattice of an ionic compound has a lot to do with the size of the ions.

For a given crystal lattice, smaller ions implies greater attraction and higher lattice energy.

LiCl and LiBr contains the same cation which is the lithium ion so we turn our attention to the anions.

Chloride ion is smaller than bromide ion, the statement LiCl > LiBr is correct based on the strength of the attractive force  bonding the ions together in each compound .

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Final answer:

The correct ranking based on ionic bond strength due to charge and size differences is LiCl > LiBr. This considers the Coulombic attraction, where a smaller ionic radius and a higher charge increase the strength of the bond.

Explanation:

The question asks to rank the strength of the attractive force bonding the ions together in each compound pair, correctly. When considering the relative strengths of ionic bonds, factors such as ionic size and charge play significant roles. The strength of an ionic bond increases with the charge of the ions and decreases with the size of the ions. Therefore, compounds with ions of higher charges and smaller sizes have stronger bonds due to the higher Coulombic attraction.

MgCl2 < CaBr2 - Incorrect because Mg2+ has a smaller ionic radius and a higher charge density than Ca2+, leading to stronger bonding in MgCl2.

LiCl > LiBr - Correct since Cl- is smaller than Br-, leading to a stronger Coulombic attraction in LiCl.

KF < KCl - Incorrect because F- is smaller than Cl-, which should result in a stronger attraction in KF due to the smaller ionic radius of F-.

NaI > Li - This comparison is not valid as it compares an ionic compound with an element.

Therefore, the correct ranking of relative strengths based on the charge and size of ions is found in option 2: LiCl > LiBr.

Answer: Option (A) is the correct answer.

Explanation:

Entropy means the degree of randomness present within the molecules of a substance.

And, in an endothermic process heat is absorbed by the reactant molecules. So, when heat is absorbed from the surroundings then there occurs a decrease in heat energy of the surrounding.

As a result, kinetic energy of surrounding elements decreases due to which there is also decrease in the entropy of surroundings.

As spontaneous process is a process that occurs on its own. So, it can be endothermic or exothermic in nature.

A state function is defined as a function that depends on the initial and final states.

Thus, we can conclude that the statement endothermic processes decrease the entropy of the surroundings, at constant T and P, is true.

None of the above statements are true. So the correct statement is E.

A. Endothermic processes decrease the entropy of the surroundings, at constant T and P.

This statement is false. Endothermic processes absorb heat from the surroundings, which can increase the entropy of the system (since disorder increases with heat transfer into the system).

At constant temperature and pressure, the entropy change of the surroundings is related to the heat absorbed or released by the system. For an endothermic process, the surroundings lose heat, which would decrease the entropy of the surroundings, not the system.

B. Endothermic processes are never spontaneous.

This statement is false. The spontaneity of a process is determined by the Gibbs free energy change (G), which depends on both the enthalpy change (H) and the entropy change (S) of the system, according to the equation G = H - TS.

An endothermic process (H > 0) can be spontaneous if the entropy increase of the system is sufficient to overcome the positive enthalpy change, particularly at high temperatures.

C. Entropy is not a state function.

This statement is false. Entropy is indeed a state function, meaning its value depends only on the initial and final states of the system and not on the path taken to go from one state to another.

This is analogous to other state functions like internal energy, enthalpy, and Gibbs free energy.

D. Exothermic processes are always spontaneous.

This statement is false. While exothermic processes (H < 0) release heat, which can contribute to spontaneity, they are not always spontaneous.

The spontaneity of an exothermic reaction also depends on the entropy change of the system.

If the entropy decrease associated with the process is large enough to result in a positive Gibbs free energy change, the process will not be spontaneous.

Therefore, since all the given statements are false, the correct answer is E. None of the above are true.

Answer:

[tex]\Delta H_{rxn3}=-162.5 kJ/mol[/tex]

Explanation:

The reaction we need to calculate:

[tex]O_3 (g) + Cl (g) \longrightarrow ClO (g) + O_2 (g)[/tex]

1) [tex]O_3 (g) + ClO (g) \longrightarrow Cl (g) +2 O_2 (g)[/tex]

[tex]\Delta H_{rxn}=-122.8 kJ/mol[/tex]

We need the ClO in the products side, so we use the inverse of this reaction:

[tex]Cl (g) +2 O_2 (g) \longrightarrow O_3 (g) + ClO (g) [/tex]

[tex]\Delta H_{rxn1}=122.8 kJ/mol[/tex]

2) [tex]2 O_3 (g) \longrightarrow 3 O_2 (g)[/tex]

[tex]\Delta H_{rxn2}=-285.3 kJ/mol[/tex]

Now we need to combine this two:

[tex]Cl (g) +2 O_2 (g) + 2 O_3 (g)\longrightarrow O_3 (g) + ClO (g) + 3 O_2 (g) [/tex]

[tex]Cl (g) + O_3 (g)\longrightarrow ClO (g) + O_2 (g) [/tex]

The enthalpy of reaction:

[tex]\Delta H_{rxn3}=\Delta H_{rxn1}+ \Delta H_{rxn2}=122.8 kJ/mol-285.3 kJ/mol[/tex]

[tex]\Delta H_{rxn3}=-162.5 kJ/mol[/tex]