Marianne gets dressed and puts on some of her favorite perfume. While applying the perfume, she accidentally gets some in her mouth and notices that it has abitter taste. After getting dressed, she heads to the kitchen to prepare some breakfast. She fills a small bowl with plain yogurt and takes a taste. The yogurt is too sour for her liking, so she adds honey to it for some sweetness. When she is done eating, she washes her bowl with soap and water. The soap is so slippery that she accidentally drops the bowl while cleaning it, causing it to break on the kitchen floor. Frustrated, Marianne sweeps up the broken glass and puts it in the trash, and then heads to work. Which substance displays a characteristic of an acid? A:soap B:yogurt C:perfume D:honey

Answer: The half reactions and net cell reaction of the cell is written below.

Explanation:

The given cell is:

[tex]Cu(s)/Cu^{2+}(aq.)||Ag^{+}(aq.)/Ag(s)[/tex]

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

Half reactions for the given cell follows:

Oxidation half reaction (anode): [tex]Cu(s)\rightarrow Cu^{2+}(aq.)+2e^-[/tex]

Reduction half reaction (cathode): [tex]Ag^{+}(aq.)+e^-\rightarrow Ag(s)[/tex]   ( × 2)

Net cell reaction:  [tex]Cu(s)+2Ag^+(aq.)\rightarrow Cu^{2+}(aq.)+2Ag(s)[/tex]

Hence, the half reactions and net cell reaction of the cell is written above.

The half-reactions at each electrode and the net cell reaction for the electrochemical cell containing copper and silver are provided.

The half-reactions at each electrode in this electrochemical cell are:

Anode: Cu (s) → Cu2+ (aq) + 2e−

Cathode: 2Ag+ (aq) + 2e− → Ag (s)

The net cell reaction for this electrochemical cell is:

Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s)

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Answer:

molarity of acid =0.0132 M

Explanation:

We are considering that the unknown acid is monoprotic. Let the acid is HA.

The reaction between NaOH and acid will be:

[tex]NaOH+HA--->NaA+H_{2}O[/tex]

Thus one mole of acid will react with one mole of base.

The moles of base reacted = molarity of NaOH X volume of NaOH

The volume of NaOH used = Final burette reading - Initial reading

Volume of NaOH used = 22.50-0.55= 21.95 mL

Moles of NaOH = 0.1517X21.95=3.33 mmole

The moles of acid reacted = 3.33 mmole

The molarity of acid will be = [tex]\frac{mmole}{volumne(mL)}=\frac{0.33}{25}=0.0132M[/tex]

The problem is about acid-base titration used in Chemistry. A 1:1 reaction between NaOH and the unknown acid is assumed. The molarity of the unknown acid is calculated as 0.1332 M.

This problem pertains to acid-base titration, a common method in Chemistry for determining the concentration of an unknown acid or base. The initial and final buret readings indicate the volume of NaOH used in the reaction: 22.50 mL - 0.55 mL = 21.95 mL, which is 0.02195 L. Using the molarity of NaOH (0.1517 M), we can find the moles of NaOH used: 0.1517 M * 0.02195 L = 0.00333 mol. Since the reaction between NaOH and the unknown acid is assumed to be 1:1, the moles of the unknown acid should also be 0.00333. Therefore, to obtain the molarity of the unknown acid, divide the moles of the acid by the volume of the acid in liters (25.0 mL = 0.025 L): 0.00333 mol / 0.025 L = 0.1332 M. Therefore, the molarity of the unknown acid is 0.1332 M.

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Answer:

Ba

Explanation:

Magnesium is the element of second group and third period. The electronic configuration of magnesium is - 2, 8, 2 or [tex]1s^22s^22p^63s^2[/tex]

There are 2 valence electrons of magnesium.

Fluorine is the element of seventeenth group and second period. The electronic configuration of fluorine is - 2, 7 or [tex]1s^22s^22p^5[/tex]

There is 1 valence electron of fluorine.

They will combine and form [tex]MgF_2[/tex]

The same type of compound is formed by the other members of the group 2 since they will have 2 valence electron.

Group 2 includes:- beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).

Hence, correct options is:- Ba

The atom that will combine with F in the same ratio as it combines with Mg is Ba.

We must recall that F combines with atoms of  elements group 2 to form ionic compounds of the sort MX2 where M is the metal.

Mg and Ba all belong to group 2 hence they will form compounds with F in the ratio of 1:2

Therefore, the atom that will combine with F in the same ratio as it combines with Mg is Ba.

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Answer:

The valid set of quantum numbers are:

a. 3,1,1,-1/2

b. 4,3,1,-1/2

c. 2,0,0,-1/2

e. 3,2,-1,-1/2

j. 3,0,0,1/2

Explanation:

Quantum numbers (n, l, mℓ, ms) are the set of numbers that describe the state of an electron in an atom.

The four quantum numbers and their rules are:

Therefore,

a. 3,1,1,-1/2: Valid

b. 4,3,1,-1/2: Valid

c. 2,0,0,-1/2: Valid

d. 1,3,0,1/2: NOT Valid

Reason: ℓ ≤ (n-1). Therefore, ℓ can not be greater than n, .

e. 3,2,-1,-1/2: Valid

f. 3,3,-1,1/2: NOT Valid

Reason: ℓ ≤ (n-1). Therefore, ℓ can not be equal to n. (ℓ ≠n)

g. 3,2,1,-1: NOT Valid

Reason: the only allowed values of ms = (- s), (+ s) = (- 1/2), (+ 1/2)

h. 1,-1,-1,-1/2: NOT Valid

Reason: ℓ ≤ (n-1) and n ≥ 1. Therefore, ℓ can not be equal to n and also ℓ can't be negative.

i. 3,3,1,1/2: NOT Valid

Reason: ℓ ≤ (n-1). Therefore, ℓ can not be equal to n. (ℓ ≠n)

j. 3,0,0,1/2: Valid

k. 4,3,4,-1/2: NOT Valid

Reason: mℓ = (- ℓ) to (+ ℓ). Therefore, mℓ can't be greater than ℓ.

l. 0,2,1,1/2: NOT Valid

Reason: n ≥ 1. Therefore, value of n can't be 0 (n≠0)

Answer: concentration in Molarity it's actually Molarity

Molarity=concentration/molar mass

Concentration=50g/0.3dm³=166.67g/dm³

Molar mass=180g/mol

Molarity=0.926mol/dm³

Answer:

Answer is =0. 925 mol L−1

Explanation:

C₆H₁₂O₆ is formula of Glucose  

For Molarity, we must know the following things  

• the number of moles of solute present in solution

• the total volume of the solution

we know the mass of one mole of Glucose = 180.156 g/mol

Number of moles = Given Mass of substance / Mass of one mole

No of moles = 50g / 180.156 g/mol

                   = 0.277 moles  

Now we know that  molarity is expressed per liter of solution. Since you dissolve 0.277 moles of potassium chloride in 300. mL of solution, you can say that 1.0 L will contain

For 300 ml of solution, no of moles are = 0.277 moles

For 1 ml of solution, no of moles are = 0.277/300 moles

For 1(1000) ml of solution, no of moles are=  0. 277/300 x 1000

                                                                 = 0.925 moles/ L

Answer is =0. 925 mol L−1

Answer:

D.) Chlorine has greater electronegativity and a larger first ionization energy

Explanation:

first we have to consider where sodium and chlorine are in the atomic table. Both are in the third row and both are nearly opposite ends of third row. sodium have high tendency to lose an electron while chlorine have higher tendency to gain an electron. so because of this fact chlorine is more electronegative than sodium.

As we move left to right in the periodic table, there is increase in the number of protons in atom and therefore there is increase in attraction between the nucleus and electrons and shrinking down the atom which is general trend when we move from left to right in the periodic table. so chlorine will be smaller than sodium because of the shrinking of the atom and smaller atoms have higher ionization energy because their electrons are close to the nucleus. They require more energy to remove. so this will make  chlorine have both a smaller atomic radius and larger ionization energy. so D is the right answer.

Final answer:

The correct statement regarding sodium and chlorine is that chlorine has a larger atomic radius and greater electronegativity.

Explanation:

The correct statement regarding sodium and chlorine is Option C: Chlorine has a larger atomic radius and greater electronegativity.

Chlorine, with 17 electrons, has a strong attraction for electrons and tends to gain an electron to form a chloride ion (Cl-). Sodium, with 11 electrons, has a lower ionization potential and tends to lose an electron to form a sodium ion (Na+). Therefore, chlorine has a greater electronegativity and a larger atomic radius compared to sodium.

Additionally, when sodium and chlorine react, sodium donates an electron to chlorine, forming an ionic bond and creating the compound sodium chloride (NaCl).

Answer:

The molarity of the Cl- anions is 0.0033 M

Explanation:

Step 1: Data given

Mass of MgCl2 = 48 mg = 48 *10^-3 grams

volume = 300 mL = 0.3L

Molar mas of MgCl2 = 95.21 g/mol

Step 2: The balanced equation

MgCl2 → Mg2+ + 2Cl-

This means for 1 mol MgCl2, we'll have 2 moles of Cl-

Step 3: Calculate moles MgCl2

Number of moles of MgCl2 = mass of MgCl2 / Molar mass of MgCl2

Moles MgCl2 = 48*10^-3 grams / 95.21 g/mol

Moles MgCl2 = 5.04 *10-4 moles

Step 4: Calculate moles of Cl-

This means for 1 mol MgCl2, we'll have 2 moles of Cl-

For  5.04 *10-4 moles MgCl2, we will have 2* 5.04 *10-4 moles = 0.001 moles Cl-

Step 5: Calculate molarity of the Cl- anion

Molarity = Moles / volume

Molarity Cl- = 0.001 moles / 0.3 L

Molarity Cl- = 0.0033 M

The molarity of the Cl- anions is 0.0033 M

Answer:

19,26 kJ

Explanation:

The work done when a gas expand with a constant atmospheric pressure is:

W = PΔV

Where P is pressure and ΔV is the change in volume of gas.

Assuming the initial volume is 0, the reaction of 500g of Zn with H⁺ (Zn(s) + 2H⁺(aq) → Zn²⁺(aq) + H₂(g)) produce:

500,0g Zn(s)×[tex]\frac{1molZn}{65,38g}[/tex]×[tex]\frac{1molH_{2}(g)}{1molZn}[/tex] = 7,648 moles of H₂

At 1,00atm and 303,15K (30°C), the volume of these moles of gas is:

V = nRT/P

V = 7,648mol×0,082atmL/molK×303,15K / 1,00atm

V = 190,1L

That means that ΔV is:

190,1L - 0L = 190,1L

And the work done is:

W = 1atm×190,1L = 190,1atmL.

In joules:

190,1 atmL×[tex]\frac{101,325}{1atmL}[/tex] = 19,26 kJ

I hope it helps!

The amount of work done against an atmospheric pressure of 1.00 atm when 500.0 g of zinc dissolves in excess acid at 30.0°C is approximately 19601.44 joules.

The amount of work done against an atmospheric pressure when a gas is produced can be calculated using the ideal gas law, which is given by PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to determine the number of moles of hydrogen gas (H2) produced from the dissolution of 500.0 g of zinc. The balanced chemical equation is:

[tex]\[ \text{Zn}(s) + 2\text{H}^+(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{H}_2(g) \][/tex]

 From the stoichiometry of the reaction, 1 mole of zinc produces 1 mole of hydrogen gas. The molar mass of zinc is approximately 65.38 g/mol. Therefore, the number of moles of zinc (n_Zn) is:

[tex]\[ n_{\text{Zn}} = \frac{\text{mass of Zn}}{\text{molar mass of Zn}} = \frac{500.0 \text{ g}}{65.38 \text{ g/mol}} \approx 7.647 \text{ mol} \][/tex]

 Since the stoichiometry is 1:1, the number of moles of hydrogen gas produced (n_H2) is also approximately 7.647 moles.

 Next, we convert the temperature from degrees Celsius to Kelvin:

[tex]\[ T = 30.0^\circ\text{C} + 273.15 = 303.15 \text{ K} \][/tex]

 Now, we can use the ideal gas law to find the volume of hydrogen gas produced at 1.00 atm of pressure:

[tex]\[ PV = nRT \][/tex]

[tex]\[ V = \frac{nRT}{P} \][/tex]

 Plugging in the values:

[tex]\[ V = \frac{(7.647 \text{ mol})(0.0821 \text{ L·atm/mol·K})(303.15 \text{ K})}{1.00 \text{ atm}} \][/tex]

[tex]\[ V \approx 193.57 \text{ L} \][/tex]

 Finally, the work done (W) against the atmospheric pressure to produce this volume of hydrogen gas is given by:

[tex]\[ W = P \cdot V \][/tex]

[tex]\[ W = 1.00 \text{ atm} \cdot 193.57 \text{ L} \][/tex]

[tex]\[ W \approx 193.57 \text{ L·atm} \][/tex]

 To express this work in joules, we use the conversion factor[tex]1 L*atm[/tex] = [tex]101.325 J:[/tex]

[tex]\[ W \approx 193.57 \text{ L·atm} \times \frac{101.325 \text{ J}}{1 \text{ L·atm}} \][/tex]

[tex]\[ W \approx 19601.44 \text{ J} \][/tex]

Therefore, the amount of work done against an atmospheric pressure of 1.00 atm when 500.0 g of zinc dissolves in excess acid at 30.0°C is approximately 19601.44 joules.

 The answer is: [tex]19601.44 \text{ J}.[/tex]

Answer:

a. strong interparticle attractions, low temperature, high pressure.

Explanation:

A gas behaves as an ideal gas when it fulfills the following conditions:

The gas deviates from the ideal behavior:

A real gas deviates most from ideal behavior under the conditions of strong interparticle attractions, low temperature, and high pressure.

A real gas deviates most from ideal behavior under the following set of conditions: strong interparticle attractions, low temperature, high pressure.

When a real gas has strong interparticle attractions, the gas particles are more likely to stick together and deviate from ideal behavior. Low temperature also contributes to the deviation as it slows down the gas particles and makes the attractive forces between them more prominent. High pressure further increases the deviation due to the decrease in empty space between the particles.

In summary, a real gas deviates most from ideal behavior when it has strong interparticle attractions, low temperature, and high pressure.

The value of ΔH is expected to be negative in processes where heat is released, which includes the condensation of steam to liquid water (II) and the freezing of water (III), both exothermic processes. Therefore, the correct answer is option D.) II and III only.

The question asks for which processes the value of ΔH (enthalpy change) is expected to be negative, indicating an exothermic reaction where heat is released. We can analyze each process one by one:

Therefore, the processes where ΔH is expected to be negative (exothermic) are options II and III, where steam condenses and water freezes.

Answer: The partial pressure of nitrogen gas is 405.76 mmHg and that of hydrogen gas is 257.24 mmHg

Explanation:

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

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

Given mass of nitrogen gas = 3.46 g

Molar mass of nitrogen gas = 28 g/mol

Putting values in above equation, we get:

[tex]\text{Moles of nitrogen gas}=\frac{3.46g}{28g/mol}=0.123mol[/tex]

Given mass of hydrogen gas = 0.156 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in above equation, we get:

[tex]\text{Moles of hydrogen gas}=\frac{0.156g}{2g/mol}=0.078mol[/tex]

Mole fraction of a gas is calculated by using the formula:

[tex]\chi_{A}=\frac{n_{A}}{n_{A}+n_{B}}[/tex]      ......(1)

Putting values in equation 1, we get:

[tex]\chi_{\text{nitrogen gas}}=\frac{0.123}{0.123+0.078}=0.612[/tex]

Putting values in equation 1, we get:

[tex]\chi_{\text{hydrogen gas}}=\frac{0.078}{0.123+0.078}=0.388[/tex]

The partial pressure of a gas is given by Raoult's law, which is:

[tex]p_A=p_T\times \chi_A[/tex]     ......(2)

where,

[tex]p_A[/tex] = partial pressure of substance A

[tex]p_T[/tex] = total pressure  = 663 mmHg

[tex]\chi_A[/tex] = mole fraction of substance A

[tex]p_{\text{Nitrogen gas}}=663mmHg\times 0.612\\\\p_{\text{Nitrogen gas}}=405.76mmHg[/tex]

[tex]p_{\text{Hydrogen gas}}=663mmHg\times 0.388\\\\p_{\text{Hydrogen gas}}=257.24mmHg[/tex]

Hence, the partial pressure of nitrogen gas is 405.76 mmHg and that of hydrogen gas is 257.24 mmHg

In this exothermic reaction, 2.50 g of hydrogen peroxide decomposes and generates -7.22 kJ of heat, as indicated by the negative sign.

The question asks for the amount of heat (q) generated when 2.50 g of hydrogen peroxide decomposes at constant pressure to give water and oxygen. Given that the enthalpy change (ΔH) for the reaction 2H2O2(l) → 2H2O(l) + O2(g) is -196 kJ, it indicates that the decomposition of hydrogen peroxide is an exothermic reaction and heat is released in the process. The negative sign of ΔH confirms this.

Firstly, we will have to find out how many moles of H2O2 are there in 2.5 g. Using the molar mass of H2O2 (34 g/mol), we get about 0.074 moles of H2O2. In the balanced chemical equation, 2 moles of hydrogen peroxide generates -196 kJ of heat. Therefore, for 0.074 moles, we calculate it by (-196 kJ * 0.074)/2 = -7.22 kJ.

The <-strong>value of q in this exothermic reaction when 2.50 g of hydrogen peroxide decomposes at constant pressure is therefore -7.22 kJ. The negative sign indicates heat is being released, or in other words, the reaction is exothermic.

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The value of q, representing the thermal energy transferred in the decomposition of 2.50g of hydrogen peroxide at constant pressure, is approximately -7.16 kJ.

The question asks for the value of q, which represents the thermal energy transferred during a reaction, in an exothermic reaction where 2.50 g of hydrogen peroxide decomposes into water and oxygen gas. In this given case, we know the enthalpy change (∆H) of the reaction is -196 kJ, indicating that this is an exothermic process where that much energy is being released to the surroundings.

We know from the balanced chemical equation 2H2O2(l) → 2H2O(l) + O2(g) that 2 moles of H2O2 decompose to release ∆H amount of energy. Let's find out the number of moles in 2.50 g of H2O2. The molar mass of H2O2 is approximately 34.01 g/mol. So, the number of moles = mass/molar mass  = 2.50 g / 34.01 g/mol = 0.0735 moles.

Considering the stoichiometry of the reaction, ∆H of -196 kJ is associated with 2 moles of H2O2. Therefore, the energy associated with 0.0735 mol will be:

q ( energy ) = ∆H x (moles of H2O2 /2) = -196 kJ x (0.0735 mol / 2 mol) = -7.1625 kJ

Therefore, the quantity of thermal energy (q) released in this decomposition reaction is approximately -7.16 kJ.

Answer:

The weight percent in the sample is 17,16%

Explanation:

The dissolution of the Ce(IV) salt provides free Ce⁴⁺ that reacts, thus:

2Ce⁴⁺ + 3I⁻ → 2Ce³⁺ + I₃⁻

I₃⁻ + 2S₂O₃²⁻ → 3I⁻ + S₄O₆²⁻

The moles in the end point of S₂O₃⁻ are:

0,01302L×0,03247M Na₂S₂O₃ = 4,228x10⁻⁴ moles of S₂O₃²⁻.

As 2 moles of S₂O₃⁻ react with 1 mole of I₃⁻, the moles of I₃⁻ are:

4,228x10⁻⁴ moles of S₂O₃⁻×[tex]\frac{1molI_{3}^-}{2molS_{2}O_{3}^{2-}}[/tex] = 2,114x10⁻⁴ moles of I₃⁻

As 2 moles of Ce⁴⁺ produce 1 mole of I₃⁻, the moles of Ce⁴⁺ are:

2,114x10⁻⁴ moles of I₃⁻× [tex]\frac{2molCe^{4+}}{1molI_{3}^-}[/tex] =  4,228x10⁻⁴ moles of Ce(IV).

These moles are:

4,228x10⁻⁴ moles of Ce(IV)×[tex]\frac{140,116g}{1mol}[/tex] = 0,05924 g of Ce(IV)

As was taken an aliquot of 25,00mL from the solution of 250,0mL:

0,05924 g of Ce(IV)×[tex]\frac{250,0mL}{25,00mL}[/tex] =0,5924g of Ce(IV) in the sample

As the sample has 3,452g, the weight percent is:

0,5924g of Ce(IV) / 3,452g × 100 = 17,16 wt%

I hope it helps!

Answer: 0.0274 M

Explanation:-

The balanced chemical solution is:

[tex]NH_4OH(aq)+HCl(aq)\rightarrow NH_4Cl(aq)+H_2O(l)[/tex]

According to the neutralization law,

[tex]n_1M_1V_1=n_2M_2V_2[/tex]

where,

[tex]M_1[/tex] = molarity of [tex]HCl[/tex] solution = 0.117 M

[tex]V_1[/tex] = volume of [tex]HCl[/tex] solution = 23.4 ml

[tex]M_2[/tex] = molarity of [tex]NH_4OH[/tex] solution = ?

[tex]V_2[/tex] = volume of [tex]NH_4OH[/tex] solution = 100.0 ml

[tex]n_1[/tex] = valency of [tex]HCl[/tex] = 1

[tex]n_2[/tex] = valency of [tex]NH_4OH[/tex] = 1

[tex]1\times 0.117M\times 23.4=1\times M_2\times 100.0[/tex]

[tex]M_2=0.0274[/tex]

Therefore, the concentration of ammonia in a solution will be 0.0274 M

Answer:

The concentration of the chemist's silver(I) nitrate  solution is  0.897 mmol/L

Explanation:

Step 1: Data given

Number of moles AgNO3 = 269 micromol = 269 * 10^-6 mol

Volume of AgNO3 = 300 mL = 0.3 L

Molar mass of AgNO3 = 169.87 g/mol

Step 2: Calculate molarity of AgNO3

Molarity = number of moles per volume (in Liters)

Molarity AgNO3 = 269 *10^-6 mol / 0.3 L

Molarity AgNO3 = 8.97 * 10^-4 M

8.97 *10^-4 mol/L = 897 micromol/L = 0.897 mmol/L

The concentration of the chemist's silver(I) nitrate  solution is  0.897 mmol/L

Final answer:

Leucine, being nonpolar, should travel farther than the polar amino acid aspartic acid on a TLC plate because nonpolar substances have a higher affinity for the stationary phase and a lower affinity for the polar mobile phase.

Explanation:

On a thin-layer chromatography (TLC) plate, the distance that a compound travels is closely related to its polarity. In this lab experiment, leucine is a nonpolar amino acid, while aspartic acid is polar due to its acidic side chain. Therefore, leucine should travel farther on the TLC plate than aspartic acid because the nonpolar amino acids have a higher affinity for the nonpolar stationary phase and a lower affinity for the polar mobile phase, so they're carried less distance by the solvent front.

The correct answer to this question is A. Leucine is nonpolar, thus it should travel farther than aspartic acid on my TLC plate.

Answer:

b. ΔE rxn is a measure of heat

Explanation:

a. ΔHrxn is the heat of reaction. TRUE. ΔHrxn or change in enthalpy of reaction is per definition the change in heat that is involved in a chemical reaction.

b. ΔErxn is a measure of heat. FALSE. Is the change in internal energy of a reaction

c. An exothermic reaction gives heat off heat to the surroundings. TRUE. An exothermic reaction is a chemical reaction that releases heat.

d. Endothermic has a positive ΔH. TRUE. When a process is exothermic ΔH<0 and when the process is endothermic ΔH>0

e. Enthalpy is the sum of a system's internal energy and the product of pressure and volume. TRUE. Under constant pressure and volume the formula is ΔH = ΔE + PV

I hope it helps!

The statement that is FALSE is b. ΔErxn is a measure of heat.

The statement that is FALSE is b. ΔErxn is a measure of heat.

ΔErxn is the change in internal energy of a system, not a direct measure of heat. It is related to heat through the equation ΔErxn = q + w, where ΔErxn is the change in internal energy, q is the heat transferred, and w is the work done on or by the system. Enthalpy, on the other hand, is a measure of heat at constant pressure, and is given by ΔHrxn = q (heat of reaction).

Therefore, option b is the false statement.

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Answer:

The molarity of HI at the equilibrium is 2.8M

Explanation:

Step 1: Data given

Volume of the flask = 250.0 mL = 0.250L

Number of moles I2 = 1.3 mol

Number of moles HI = 1.0 mol

Kc = 0.983

Step 2: The balanced equation

H2(g) +I2(g) ⇆ 2HI(g)

For 1 mole I2 consumed, we need 1 mole H2 to produce 2 moles HI

Step 3: Calculate initial concentrations

Initial concentration I2 = 1.3mol / 0.25L

Initial concentration I2 = 5.2 M

Initial concentration HI = 1.0 mol / 0.25L

Initial concentration HI = 4.0 M

Step 4: Calculate concentrations at equilibrium

The concentration at equilibrium is:

[I2] = (5.2+x)M

[HI] = (4.0 - x)M

[H2] = xM

Kc = [HI]²/[H2][I2]

0.983 = (4-x)²/ (x*(5.2+x))

0.983 = (4-x)²/ (5.2x +x²)

5.1116x + 0.983 x² = 16 -8x +x²

-0.017x² +13.1116x -16 = 0

x = 1.222 = [H2]

[HI] = 4.0 - 1.222 = 2.778M ≈ 2.8 M

[I2] = 5.2 + 1.222 = 6.422 M ≈ 6.4 M

To control we can calculate:

[2.778]² / [1.222][6.422]  = 0.983 = Kc

The molarity of HI at the equilibrium is 2.8M

Final answer:

The weight percent of NH3 in the aqueous waste was calculated from the titration data to be 0.2047%. The moles of NH3 were found to be 0.0029711 mol, corresponding to 0.050585g NH3 in the original waste sample.

Explanation:

The weight percent of NH3 in the aqueous waste is calculated using titration analysis. First, determine the moles of HCl that reacted:
# mol HCl = 0.02842 L × 0.1045 M = 0.0029711 mol HCl.

The reaction between HCl and NH3 is:
NH3(aq) + HCl(aq) → NH4Cl(aq).

Hence, 1 mole of HCl reacts with 1 mole of NH3. Therefore, the moles of NH3 in the aliquot are also 0.0029711 mol. To find the mass of NH3:
Mass of NH3 = moles × molar mass
              = 0.0029711 mol × 17.031 g/mol
              = 0.050585 g NH3.

Since the aliquot is part of the diluted waste, and assuming the ammonia is evenly distributed, we calculate the weight percent in the original waste sample:
   Weight percent = (mass of NH3 in aliquot / mass of waste sample) × 100
                 = (0.050585 g / 24.711 g) × 100
                 = 0.2047%.

Answer:

mass of O₂ = 800 g

Explanation:

Formula of Octane = C₈H₁₈

Formula of Oxygen = O₂

Balanced Chemical Reaction:

Octane react with oxygen and produce water and carbon dioxide.

                    2C₈H₁₈ + 25O₂ ---------> 16CO₂+ 18H₂O

Moles calculation:

From the number of moles of the reactant used in a chemical reaction specific number of product produced. we can find the amount of any reactant and product from the mole ratio of a chemical reaction.

Mole formula =  

no. of moles = mass in grams / molecular mass ............... (1)

Given Data:

Molecular Weight of O₂  =  (16 x2 ) = 32 g/mol

Mass of O₂ = To be find

Calculations:

                             2C₈H₁₈  +  25O₂      --------->  16CO₂   +    18H₂O

                              2mole      25 mole                 16 mole     18 mole

From the above balanced chemical equation it is know that 2 mole of octane consume 25 mole of oxygen.

so we have to calculate the mass of oxygen that is consumed

by using mole formula  (1) we can fine the mass of oxygen

we know

Molecular Weight of O₂  =  32 g/mol

number of moles of Oxygen molecule = 25 mol

putting the value in the below formula

            no. of moles of O₂ = mass of O₂ / molecular mass of O₂

            25 mole = mass of O₂ / 32 g/mol ....... (2)

By rearragming the equation (2)

            mass of O₂ = 25 mole x 32 g/mol

            mass of O₂ = 25 mole x 32 g/mol

            mass of O₂ = 800 g

So in the octan reaction with oxygen 800g of oxygen will use.  

Answer: d) ΔS is positive and ΔH is negative

Explanation:

According to Gibb's equation:

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

[tex]\Delta G[/tex] = Gibbs free energy  

[tex]\Delta H[/tex] = enthalpy change

[tex]\Delta S[/tex] = entropy change  

T = temperature in Kelvin

[tex]\Delta G[/tex]= +ve, reaction is non spontaneous

[tex]\Delta G[/tex]= -ve, reaction is spontaneous

[tex]\Delta G[/tex]= 0, reaction is in equilibrium

a)  ΔS is negative and ΔH is positive

[tex]\Delta G=(-ve)-T(+ve)[/tex]

[tex]\Delta G=(-ve)(-ve)=-ve[/tex]  

Reaction is spontaneous at all temperatures.

b) ΔS is positive and ΔH is positive

[tex]\Delta G=(+ve)-T(+ve)[/tex]

[tex]\Delta G=(+ve)(-ve)=-ve[/tex]  

Reaction is spontaneous at high temperatures.

c) ΔS is negative and ΔH is negative

[tex]\Delta G=(-ve)-T(-ve)[/tex]

[tex]\Delta G=(-ve)(+ve)=-ve[/tex]  

Reaction is spontaneous at low temperatures.

d) ΔS is positive and ΔH is negative

[tex]\Delta G=(+ve)-T(-ve)[/tex]

[tex]\Delta G=(+ve)(+ve)=+ve[/tex]  

Reaction is non spontaneous or thermodynamically unfavored at all temperatures.

Answer: The standard cell potential of the cell is -0.71 V

Explanation:

The half reactions follows:

Oxidation half reaction:  [tex]Mg\rightarrow Mg^{2+}+2e^-;E^o_{Mg^{2+}/Mg}=-2.37V[/tex]  ( × 3)

Reduction half reaction:  [tex]Al^{3+}(aq.)+3e^-\rightarrow Al(s);E^o_{Al^{3+}/Al}=-1.66V[/tex]  ( × 2)

The balanced cell reaction follows:

[tex]2Al^{3+}(aq.)+3Mg(s)\rightarrow 2Al(s)+3Mg^{2+}(aq.)[/tex]

To calculate the [tex]E^o_{cell}[/tex] of the reaction, we use the equation:

[tex]E^o_{cell}=E^o_{cathode}-E^o_{anode}[/tex]

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

Putting values in above equation, we get:

[tex]E^o_{cell}=-2.37-(-1.66)=-0.71V[/tex]

Hence, the standard cell potential of the cell is -0.71 V

The final temperature of the mixture is approximately [tex]\(-57.97^\circ\text{C}\)[/tex].

To find the final temperature of the mixture, we can use the principle of conservation of energy, assuming no heat is lost or gained in the process.

The heat gained by the cold substance (water) will be equal to the heat lost by the hot substance (ethanol).

The heat gained or lost [tex](\(Q\))[/tex] can be calculated using the equation:

[tex]\[ Q = mc\Delta T \][/tex]

where:

- [tex]\(m\)[/tex] is the mass of the substance,

- [tex]\(c\)[/tex] is the specific heat capacity of the substance,

- [tex]\(\Delta T\)[/tex] is the change in temperature.

The sum of the heats gained and lost is zero:

[tex]\[ Q_{\text{water}} + Q_{\text{ethanol}} = 0 \][/tex]

Since the final temperature is the same for both substances, we can write the equation:

[tex]\[ m_{\text{water}}c_{\text{water}}\Delta T_{\text{water}} + m_{\text{ethanol}}c_{\text{ethanol}}\Delta T_{\text{ethanol}} = 0 \][/tex]

Rearrange the equation to solve for the final temperature [tex](\(T_{\text{final}}\))[/tex]:

[tex]\[ \Delta T_{\text{water}} + \Delta T_{\text{ethanol}} = 0 \][/tex]

[tex]\[ T_{\text{final}} - T_{\text{initial, water}} + T_{\text{final}} - T_{\text{initial, ethanol}} = 0 \][/tex]

[tex]\[ 2T_{\text{final}} = T_{\text{initial, water}} + T_{\text{initial, ethanol}} \][/tex]

[tex]\[ T_{\text{final}} = \frac{T_{\text{initial, water}} + T_{\text{initial, ethanol}}}{2} \][/tex]

Now, substitute the given values:

[tex]\[ T_{\text{final}} = \frac{(55.0 \ \text{mL} \times 1.0 \ \text{g/mL} \times 4.18 \ \text{J/g}^\circ\text{C} \times (28.6^\circ\text{C} - T_{\text{final}})) + (55.0 \ \text{mL} \times 0.789 \ \text{g/mL} \times 2.44 \ \text{J/g}^\circ\text{C} \times (T_{\text{final}} - 9.0^\circ\text{C}))}{2} \][/tex]

[tex]\[ T_{\text{final}} = \frac{(55.0 \ \text{mL} \times 4.18 \ \text{J/g}^\circ\text{C} \times (28.6^\circ\text{C} - T_{\text{final}})) + (55.0 \ \text{mL} \times 0.789 \ \text{g/mL} \times 2.44 \ \text{J/g}^\circ\text{C} \times (T_{\text{final}} - 9.0^\circ\text{C}))}{2} \][/tex]

Combine like terms:

[tex]\[ T_{\text{final}} = \frac{(55.0 \times 4.18 \times 28.6) + (55.0 \times 0.789 \times 2.44 \times (T_{\text{final}} - 9.0))}{2} \][/tex]

[tex]\[ T_{\text{final}} = \frac{(6132.86 + 107.79 \times (T_{\text{final}} - 9.0))}{2} \][/tex]

[tex]\[ T_{\text{final}} = \frac{6132.86 + 107.79T_{\text{final}} - 971.1}{2} \][/tex]

[tex]\[ 2T_{\text{final}} = 7101.76 + 107.79T_{\text{final}} - 971.1 \][/tex]

Combine like terms:

[tex]\[ 2T_{\text{final}} - 107.79T_{\text{final}} = 7101.76 - 971.1 \][/tex]

[tex]\[ -105.79T_{\text{final}} = 6130.66 \][/tex]

[tex]\[ T_{\text{final}} \approx -57.97^\circ\text{C} \][/tex]

Therefore, the final temperature of the mixture is approximately [tex]\(-57.97^\circ\text{C}\)[/tex]. This negative value indicates that the final temperature is lower than the initial temperatures of water and ethanol, which is consistent with the fact that heat is transferred from the substances with higher initial temperatures to the one with a lower initial temperature.

Answer:

The concentration of the H₃PO₄ solution is 0,245M

Explanation:

The first titration is:

KHP + NaOH → KP⁻ + Na⁺ + H₂O

0,495g of KHP are:

0,495g×[tex]\frac{1mol}{204,22g}[/tex]= 2,42x10⁻³ moles of KHP

As 1 mole of KHP reacts with 1 mole of NaOH, moles of NaOH are 2,42x10⁻³ moles.

As volume required was 28,56mL, the concentration of the NaOH solution is:

2,42x10⁻³ moles / 0,02856L = 0,0849M

The titration of the phosporic acid with NaOH occurs as follows:

H₃PO₄ + NaOH → H₂PO₄⁻ + Na⁺ + H₂O

If were required 29,88mL of NaOH, the moles of NaOH spent were:

0,0849M×0,02988L = 2,54x10⁻³ moles of NaOH that are the same than H₃PO₄ moles.

As the volume of the solution of H₃PO₄ was 10,33mL, the concentration of the H₃PO₄ solution is:

2,54x10⁻³ moles of H₃PO₄ / 0,01033L = 0,245M

I hope it helps!

Final answer:

The concentration of the phosphoric acid is calculated using the molarity of a standardized NaOH solution obtained from a titration with KHP. The determined NaOH molarity is then applied to find the moles of phosphoric acid reacted in its own titration, which leads to the final concentration of the acid.

Explanation:

To determine the concentration of the phosphoric acid (H3PO4), we first need to calculate the molarity of the sodium hydroxide (NaOH) solution using the titration with potassium hydrogen phthalate (KHP). Since 0.495 grams of KHP was titrated with 28.56 mL of NaOH, we can calculate the moles of KHP used:

Now, using the concentration of NaOH, we can find the concentration of phosphoric acid. Given that 29.88 mL of the NaOH solution is required to titrate the 10.33 mL of H3PO4, we have:

Answer:

V= 0.544

Explanation:

Given that

σ=812 MPa

σ₁=1240 MPa

σ₂=300 MPa

Lets take volume fraction V

The strength of composite fiber given as

σ = σ₁ V + σ₂(1-V)

By putting the values

812 = 1240 V + 300 (1-V)

812 = 1240 V +300 - 300 V

812 - 300 = 1240 V- 300 V

512 = 940 V

V= 0.544

The percentage volume = 54.4 %

Answer:

The molar solubility of distilled water is [tex]$1.25 \times 10-3$[/tex] (Option B)

Explanation:

Given:

[tex]Pbl_2 -7.9 \times 10^-^9.[/tex]

Expression for solubility constant is,

[tex]$K_{s p}=\left[P b^{2+}\right]\left[I^{-}\right]^{2}$[/tex]

The given equation is,

[tex]$K_{s p}=7.9 \times 10^{-9}$[/tex]

Equation is to calculated as,  

[tex]$7.9 \times 10^{-9}=(s) \times(2 s)^{2}$[/tex]

[tex]$7.9 \times 10^{-9}=4 s^{3}$[/tex]

[tex]$s=1.25 \times 10^{-3} \mathrm{~mol} / L$[/tex]

The solubility product in distilled water is [tex]$s=1.25 \times 10^{-3} \mathrm{~mol} / L$[/tex].

Learn more about bonds refer:

The correct answer is C.)[tex]5.0x10^-^4.[/tex]

To determine the molar solubility of PbI2 in distilled water, we need to use the solubility product constant (Ksp) for PbI2, which is given as 7.9x10^-9.

 The chemical equation for the dissociation of PbI2 in water is:

[tex]\[ PbI_2(s) \rightleftharpoons Pb^{2+}(aq) + 2I^-(aq) \][/tex]

 The solubility product expression for this equilibrium is:

[tex]\[ Ksp = [Pb^{2+}][I^-]^2 \][/tex]

Let's denote the molar solubility of PbI2 as s. This means that the concentration of Pb^2+ ions will be s, and the concentration of I^- ions will be 2s (since 2 moles of I^- are produced for every mole of PbI2 that dissolves). We can now express the Ksp equation in terms of s:

[tex]\[ Ksp = s \cdot (2s)^2 \][/tex]

[tex]\[ Ksp = s \cdot 4s^2 \][/tex]

[tex]\[ Ksp = 4s^3 \][/tex]

 Now we can solve for s using the given Ksp value:

[tex]\[ 7.9 \times 10^{-9} = 4s^3 \][/tex]

[tex]\[ s^3 = \frac{7.9 \times 10^{-9}}{4} \][/tex]

[tex]\[ s^3 = 1.975 \times 10^{-9} \][/tex]

[tex]\[ s = \sqrt[3]{1.975 \times 10^{-9}} \][/tex]

[tex]\[ s \approx 5.82 \times 10^{-4} \][/tex]

 Since we are looking for the molar solubility, we can round this value to the appropriate number of significant figures, which is two significant figures based on the Ksp value given [tex](7.9x10^-9[/tex] has two significant figures). Therefore, the molar solubility of PbI2 in distilled water is approximately:

[tex]\[ s \approx 5.8 \times 10^{-4} \][/tex]

 The closest answer choice to this calculated value is C.) 5.0x10^-4.

Answer:

ΔU = -538kJ/mol

Explanation:

Step 1: Data given

Mass of compound X = 0.485 grams

Mass of water = 3000 grams

Temperature rise = 0.285 °C

Heat capacity of the calorimeter = 3.81 kJ/°C

Specific heat of water = 4.184 J/g°C

MW of X = 56.0 g/mol

Step 2: Calculate q

∆U = ΔH - PΔV

Since the bomb calorimeter has a constant volume  ΔV = 0

⇒ ΔU = ΔH

qrxn = - (q(water) + q(bomb))

q(bomb) = 3810 J/°C * 0.285 = 1085.85 J

q(water) = 3000g * 4.184 J/g°C * 0.285°C = 3577.32 J

qrxn = q(water) + q(bomb)

qrxn = 4663.17 J = 4.66 kJ (Since this is an exothermic, the heat is released. (q is positive, ΔH is negative).

Step 3: Calculate moles of compound

Moles = mass / molar mass

Moles = 0.485 grams / 56.0 g/mol

Moles = 0.00866 moles

Step 4: Calculate ΔU

= 4663.17 J /0.00866 moles = 538472 j/mol = 538.5 kJ/mol

Since the reaction is exothermic, ΔU is negative

ΔU = -538kJ/mol

Answer:

0.238 M

Explanation:

A 17.00 mL sample of the dilute solution was found to contain 0.220 M ClO₃⁻(aq). The concentration is an intensive property, so the concentration in the 52.00 mL is also 0.220 M ClO₃⁻(aq). We can find the initial concentration of ClO₃⁻ using the dilution rule.

C₁.V₁ = C₂.V₂

C₁ × 24.00 mL = 0.220 M × 52.00 mL

C₁ = 0.477 M

The concentration of Pb(ClO₃)₂ is:

[tex]\frac{0.477molClO_{3}^{-} }{L} \times \frac{1molPb(ClO_{3})_{2}}{2molClO_{3}^{-}} =0.238M[/tex]

Answer:

a. 1,157x10⁻⁵M/s

b. 5,787x10⁻⁶M/s

Explanation:

For the reaction:

2H₂O₂(aq) → 2H₂O(l) + O₂(g).

a. The rate law of descomposition is:

[tex]rate=-\frac{1}{2} \frac{d[H_{2}O_{2}]}{dt}=\frac{d[O_{2}]}{dt}[/tex]

Where d[H₂O₂] is the change in concentration of H₂O₂ (between 0s and 2,16x10⁴s) is (1,000M-0,500M) and dt is (0s-2,16x10^4s). Replacing:

[tex]rate=-\frac{1}{2} \frac{0,500M}{-2,16x10^4s}[/tex]

[tex]rate=1,157x10^{-5}M/s[/tex]

As this rate is = d[O₂]/dt(Rate of production of O₂), the rate of production of O₂(g) is 1,157x10⁻⁵M/s

b. Between 2,16x10⁴s and 4,32x10⁴s, rate law is:

[tex]rate=-\frac{1}{2} \frac{0,500M-0,250M}{2,16x10^4s-4,32x10^4s}[/tex]

[tex]rate=5,787x10^{-6}M/s[/tex]

The rates are 5,787x10⁻⁶M/s

I hope it helps!

The study of chemicals and bonds is called chemistry. There are two types of elements these rare metals and nonmetals.

Thus the rate is,

[tex]rate=1157\times10^{-5}[/tex]

The rate law or rate equation for a chemical reaction is an equation that links the initial or forward reaction rate with the concentrations or pressures of the reactants and constant parameters.

The balanced reaction is:-

[tex]2H_2O_2(aq)----->2H_2O(l)+o_2(g)[/tex]

The rate law of decomposition:-

[tex]rate=-\dfrac{1}{2}\dfrac{d[H_2O_2]}{dt}[/tex]

Where d[H₂O₂] is the change in concentration of H₂O₂ (between 0s and 2,16x10⁴s) is (1,000M-0,500M) and dt is (0s-2,16x10^4s). Replacing:

[tex]rate=-\dfrac{1}{2}\dfrac{0.5}{2.16\times10^{4}}[/tex]

[tex]rate=1157\times10^{-5}[/tex]

As this rate is = d[O₂]/dt(Rate of production of O₂), the rate of production of O₂(g) is 1,157x10⁻⁵M/s

For more information about the rate of reaction, refer to the link:-

brainly.com/question/16759172

Answer:

The calcium chloride is an electrolyte salt, so the frezzing point of solution must be higher than ethylene glycol.

Explanation:

This is the colligative property for this question: Frezzing point depression

ΔTf = Kf · molal · i

ΔTf = T° fussion solvent pure - T° fussion solution

As both solutions are the same in molality and the solvent is water, the formula stands the same but the Calcium Chloride is a salt which is dissociated in water like this:

CaCl₂ → Ca²⁺  + 2Cl⁻

We have 3 moles of ions, so this value modiffy the formula with the Van't Hoff Factor (number of ion particles per individual molecule of solute).

Ethyleneglycol  is a non-electrolytic organic compound (It is often used 1 as the i).

Let's see the formula in both:

0° - T° fussion solution = Kf · molal · 3 → CaCl2

0° - T° fussion solution = Kf · molal · 1 → C2H6O2