0.20 mol solute 0.300 kg solvent
calculate the molality of the solution

Answer:

The answers that represent a decrease in entropy are:

-CO2 gas is dissolved in water to make a carbonated beverage

-NO2(g) → N2O4(g)

Explanation:

Since in carbonated drinks, carbon dioxide is in its liquid form, since a pressure is applied to said gas, in this way, when carbon dioxide dissolves in a liquid, its entropy decreases, thus producing a negative change in entropy (the entropy of a gas is higher than the entropy of a liquid).

The number of gaseous reagents is equal to 1-2 = -1. Since it is negative, therefore, entropy is also negative.

Answer:

28.5 L of Cl

Explanation:

From PV=nRT

P= 794torr or 1.04 atm

T= 625°C or 898K

R= 0.0821 L atm mol−1 K−1

n= 3 moles

V= ???

V= nRT/P

V=3× 0.0821× 898/1.04

V= 212.7 L

From the balanced reaction equation

112g of iron reacted with 212.7L of Cl

15.0 g of iron will react with 15.0×212.7/112

= 28.5 L of Cl

Answer:

No, it is not.

Explanation:

Most solutions do not behave ideally. Designating two volatile  substances as A and B, we can consider the following two cases:

Case 1: If the intermolecular forces between A and B molecules are weaker than  those between A molecules and between B molecules, then there is a greater tendency  for these molecules to leave the solution than in the case of an ideal solution. Consequently,  the vapor pressure of the solution is greater than the sum of the vapor  pressures as predicted by Raoult’s law for the same concentration. This behavior gives  rise to the positive deviation.

Case 2: If A molecules attract B molecules more strongly than they do their own  kind, the vapor pressure of the solution is less than the sum of the vapor pressures as  predicted by Raoult’s law. Here we have a negative deviation.

The benzene/toluene system is an exception, since that solution behaves ideally.

No, in the case of an ideal solution of two volatile liquids the two substances at different state cannot coexist for a single value of pressure at a given temperature.

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Answer:

0.1472 mol/L is the concentration of the barium hydroxide solution.

Explanation:

[tex]2KHC_8H_4O_4+Ba(OH)_2\rightarrow Ba(KC_8H_4O_4)_2+2H_2O[/tex]

Mass of potassium hydrogen phthalate = 2.050 g

Molar mass of potassium hydrogen phthalate = [tex]\frac{2.050 g}{204.2 g/mol}=0.01004 mol[/tex]

According to reaction , 2 moles of potassium hydrogen phthalate reacts with 1 mole of barium hydroxide, then 0.01004 moles of potassium hydrogen phthalate will :

[tex]\frac{1}{2}\times 0.01004 mol=0.005020 mol[/tex] of barium hydroxide

Moles of barium hydroxide = 0.005020 mol

Volume of the barium hydroxide solution = 34.10 mL = 0.03410 L

1 mL = 0.001 L

[tex]Molarity=\frac{Moles}{Volume(L)}[/tex]

Molarity of the barium hydroxiude silution :

[tex]=\frac{0.005020 mol}{0.03410 L}=0.1472 mol/L[/tex]

0.1472 mol/L is the concentration of the barium hydroxide solution.

Answer:

7.26 moles of NH₃ are formed in this reaction

Explanation:

This is about the reaction for the production of ammonia

1 mol of nitrogen gas reacts to 3 moles of hydrogen in order to produce 2 moles of ammonia.

The equation is: N₂ + 3H₂ → 2NH₃

In the question, we were informed that the excess is the H₂ so the N₂ is limiting reagent. We determine the moles, that has reacted:

101.7 g / 28 g/mol = 3.63 moles

So, If 1 mol of nitrogen gas can produce 2 moles of ammonia

3.63 moles of N₂ must produce ( 2 . 3.63) / 1 = 7.26 moles of NH₃

Answer:

In this reaction, 7.26 moles of NH3 will be formed.

Explanation:

Step 1: Data given

Mass of N2 = 101.7 grams

Molar mass N2 = 28.0 g/mol

H2 is in excess

Molar mass H2 = 2.02 g/mol

Molar mass of NH3 = 17.03 g/mol

Step 2: The balanced equation

N2(g) + 3H2(g) → 2NH3(g)

Step 3: Calculate moles N2

Moles N2 = mass N2/ molar mass N2

Moles N2 = 101.7 grams / 28.0 g/mol

Moles N2 = 3.63 moles

Step 4: Calculate moles NH3

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

For 3.63 moles N2 we'll produce2*3.63 = 7.26 moles NH3

In this reaction, 7.26 moles of NH3 will be formed.

Final answer:

The true statements about particle motion and temperature are that the average kinetic energy of the particles in a substance determines its temperature and that faster moving particles generally result in a higher temperature of the substance.

Explanation:

The relationship between particle motion and temperature is based on the kinetic-molecular theory. According to this theory, temperature is proportional to the average kinetic energy of the particles, such as molecules or atoms, in a substance. Therefore:

The average kinetic energy of the particles in a substance determines the substance's temperature.

If the particles in two pure substances have the same average speed, it does not necessarily mean they have the same temperature, since heavier particles will have more kinetic energy at the same speed, leading to different temperatures.

When two substances have the same temperature, it indicates that the average kinetic energy of the particles in both substances is the same, not that all of the particles are moving at the same speed, because particles have a range of speeds.

The speed of a substance's particles can give an indication of how hot or cold that substance is. Faster moving particles generally mean a higher temperature.

As such, the true statements are 1 and 4. Understanding that temperature is not simply a measure of particle speed, but rather the average kinetic energy involved, clarifies misconceptions about the nature of thermal energy and its measurement.

Answer:

I should use a volumetric flask.

Explanation:

If the accuracy of the concentration is important, we need to use a volumetric flask.

Answer:

The glassware appropriate for dilution preparation is a (250 mL) volumetric flask

Explanation:

We know that molarity or concentration of a solution is the number of moles per litres of solution,  the molarity and volume of the solution in question can be used to find out how much of the stock solution to be diluted using the formula;

[tex]c = \frac{n}{v}[/tex]

Once the variables are confirmed, a 250 mL solution of 1.50M HCl can be prepared by measuring determined stock solute into a 250mL volumetric flask and the making it upto the 250mL mark. (a measuring cylinder can be used to check accuracy of volume added).

The dissolution of potassium hydroxide (KOH) in water is an exothermic process, as indicated by the increase in temperature when KOH is dissolved in water.

The dissolution of potassium hydroxide (KOH) in water is an exothermic process. This can be determined based on the observation that the temperature of the water increased from 23.0°C to 34.0°C when 11.1 g of KOH was dissolved in 250.0 g of water. The positive change in temperature indicates that heat was released by the KOH dissolving in water, resulting in an increase in temperature.

The reaction is exothermic as the temperature of the water rises from 23.0°C to 34.0°C, indicating the release of heat.

To determine if the reaction is exothermic or endothermic, we need to look at the temperature change during the dissolution of potassium hydroxide (KOH).

Since the temperature of the water rises from 23.0 °C to 34.0 °C, which is an increase of 11.0 °C, this indicates that the solution absorbs heat.

This increase in temperature demonstrates that the reaction releases heat into the surroundings, thus it is an exothermic reaction. In an exothermic reaction, the temperature of the surroundings rises because energy is released.

Example Calculation:

Mass of water (m): 250 g

Specific heat capacity (C) of water: 4.184 J/g°C

Temperature change (ΔT): 34.0 °C - 23.0 °C = 11.0 °C

Heat (q) absorbed by the solution: q = m × C × ΔT = 250 g × 4.184 J/g°C × 11.0 °C = 11, 506 J or 11.506 kJ

Since the heat is released by the dissolution of KOH, the reaction is said to be exothermic.

Complete Question

To make use of an ionic hydrate for storing solar energy, you place 422.0 kg of sodium sulfate decahydrate on your house roof. Assuming complete reaction and 100% efficiency of heat transfer, how much heat (in kJ) is released to your house at night? Note that sodium sulfate decahydrate will transfer 354 kJ/mol.

Answer:

The amount of energy released is [tex]x = 4.63650 *10^5 KJ[/tex]

Explanation:

Number of moles is mathematically represented as

                         [tex]n =\frac{mass}{Molar\ Mass}[/tex]

substituting [tex]422.0kg = 422 *10^3g[/tex] for mass of sodium sulfate decahydrate([tex]Na_2 SO_4 \cdot 10H_2 O[/tex]), [tex]322.2g/mol[/tex] (This value is a constant )for the molar mass of sodium sulfate decahydrate

                        [tex]n= \frac{422*10^3}{322.2}[/tex]

                           [tex]= 1309.7 \ moles[/tex]

From the question we are told that

            1 mole of sodium sulfate decahydrate generates [tex]354KJ[/tex] of energy

         So  1309.7 mole would generate  x

Now stating the relation mathematically

                 1 mol → 354KJ

                 1309.7 mol → x

=>      [tex]x = 4.63650 *10^5 KJ[/tex]

Answer:

The solution will turn red.  

Explanation:

HC₁₄H₁₄SO₃ + H₂O ⇌ HC₁₄H₁₄SO₃⁻ +H₃O⁺

     (red)                           (yellow)

Methyl orange is a weak acid in which the ionized and unionized forms are distinct colours and are in equilibrium with each other,

At about pH 3.4,  the two the forms are present in equal amounts, and the indicator colour is orange.

If you add more acid, you are disturbing the equilibrium.

According to Le Châtelier's Principle, when you apply a stress to a system at equilibrium, it will respond in such a way as to relieve the stress.

The system will try to get rid of the added acid, so the position of equilibrium will move to the left.

More of the unionized molecules will form, so the solution will turn red.

Answer:

Molality = 6.0 m

Explanation:

The molecular weight of tartaric acid = 150.087 g/mol

Given that:

Density  of the solution = 1.023 g/mL

Molarity =  3.23M

Density is given as : [tex]Molarity ( \frac{1}{molality } +\frac{mol.wt}{1000} )[/tex]

∴

[tex]1.023 = 3.23 (\frac{1}{molality } +\frac{150.087}{1000} )[/tex]

[tex]\frac{1}{molality } =( \frac{1.023}{3.23} - \frac{150.087}{1000} )[/tex]

[tex]\frac{1}{molality } =0.3167 - 0.1500[/tex]

[tex]\frac{1}{molality } = 0.1667[/tex]

Molality  = [tex]\frac{1}{0.1667}[/tex]

Molality = 5.999 m

Molality ≅ 6.0 m

Answer:

V= 9.45L

Explanation:

P=3.75atm, V=?, n= 1.5, R= 0.082, T= 15+ 273= 288K

Applying

PV= nRT

Substitute and Simplify

3.75*V= 1.5*0.082*288

V= 9.45L

The approximate volume of a 1.50 mol sample of gas at 15.0°C and a pressure of 3.75 atm is calculated using the Ideal Gas Law to be about 9.20 liters.

To calculate the approximate volume of a 1.50 mol sample of gas at 15.0°C and a pressure of 3.75 atm, we can use the Ideal Gas Law, which is PV = nRT. First, we must convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. Then we can solve for V, the volume of the gas.

The conversion from Celsius to Kelvin: T(K) = 15.0 + 273.15 = 288.15 K

Using the Ideal Gas Law constants, R = 0.0821 L·atm/K·mol. Substituting the known values into the Ideal Gas Law equation:

PV = nRT
(3.75 atm) × V = (1.50 mol) × (0.0821 L·atm/K·mol) × (288.15 K)

V = (1.50 mol × 0.0821 L·atm/K·mol × 288.15 K) / 3.75 atm

V = 9.2029 L

Therefore, the approximate volume of the gas sample is about 9.20 liters.

Answer: This reaction is never spontaneous

Explanation:

According to Gibbs equation:

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

[tex]\Delta G[/tex] = Gibb's free energy change

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

T = temperature

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

A reaction becomes spontaneous when [tex]\Delta G[/tex] = Gibb's free energy change is negative.

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

[tex]\Delta G=+ve+ve[/tex]

[tex]\Delta G=+ve[/tex]

Thus this reaction is never spontaneous

Answer:

See explaination

Explanation:

We can define the Diels-Alder reaction as a conjugate addition reaction of a conjugated diene to an alkene (the dienophile) to produce a cyclohexene.

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The Diels–Alder reaction is an organic chemistry reaction involving a cyclic rearrangement of atoms to form a six-membered ring. The product structure from such a reaction should specify stereochemistry with wedge-and-dash notation for the chirality centers involving carbon atoms and Deuterium (D). A wedge implies the bond is positioned towards you, while a dash implies the bond is positioned away from you.

This is a Chemistry problem dealing with the Diels–Alder reaction, a fundamental reaction in organic chemistry, which is a very key method in the synthesis of complex molecules. In essence, the Diels–Alder reaction involves a cyclic rearrangement of atoms rearranging to form a six-membered ring. Let's take a Diels–Alder reaction template where:

two carbon atoms involved in the double bond are labeled as X and Y,

the carbonyl carbon is labeled as Z,

the specific hydrogen atom replaced by Deuterium (D) is labeled as W.

Thus, when a Diels–Alder reaction is performed, the product structure will maintain relative positions. Carbon atoms X and Z will have wedge orientation while Carbon atoms Y and the Deuterium (D) on W will have dash orientation.

Remember, in wedge-and-dash notation, wedge implies the bond is coming up out of the plane (positioned towards you), while dash implies the bond is going back into the plane (positioned away from you).

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Answer:

A the reaction will form

Explanation:

Answer : The electronic geometry and the molecular geometry of the molecule will be octahedral.

Explanation :

Formula used  :

[tex]\text{Number of electron pair}=\frac{1}{2}[V+N-C+A][/tex]

where,

V = number of valence electrons present in central atom

N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

The given molecule is, [tex]PF_6^-[/tex]

[tex]\text{Number of electrons}=\frac{1}{2}\times [5+6+1]=6[/tex]

The number of electron pair are 6 that means the hybridization will be [tex]sp^3d^2[/tex] and the electronic geometry and the molecular geometry of the molecule will be octahedral.

The correct number of regions of electron density around the central atom in PF₆- is 6. The electronic geometry of PF6- is octahedral, and the molecular geometry is also octahedral.

To determine the number of electron regions around the central phosphorus atom in PF6-, we count the bonded atoms and any lone pairs on the central atom.

The Lewis structure of PF6- shows that the phosphorus atom is bonded to six fluorine atoms and has no lone pairs since it is surrounded by six bonding groups and has a formal charge of -1, which balances the overall charge of the ion.

Each bonded fluorine contributes one region of electron density, and there are no lone pairs on the phosphorus atom.

Therefore, there are six regions of electron density around the central phosphorus atom, which corresponds to an octahedral electronic geometry.

 Since there are no lone pairs, the molecular geometry is the same as the electronic geometry, which is octahedral. This means that all six fluorine atoms are arranged around the central phosphorus atom in a way that they are at the vertices of an octahedron.

 In summary, the VSEPR theory predicts that PF6- has six regions of electron density, an octahedral electronic geometry, and an octahedral molecular geometry.

Answer:

4.65 L of NH₃ is required for the reaction

Explanation:

2NH₃(g)  +  H₂SO₄(aq)  → (NH₄)₂SO₄(s)

We determine the ammonium sulfate's moles that have been formed.

8.98 g . 1mol / 132.06 g = 0.068 moles

Now, we propose this rule of three:

1 mol of ammonium sulfate can be produced by 2 moles of ammonia

Therefore, 0.068 moles of salt were produced by (0.068 . 29) / 1 = 0.136 moles of NH₃. We apply the Ideal Gases Law, to determine the volume.

Firstly we do unit's conversions:

27.6°C +273 =  300.6 K

547.9 mmHg . 1 atm / 760 mmHg = 0.721 atm

V = ( n . R . T ) / P → (0.136 mol . 0.082 L.atm/mol.K . 300.6K) / 0.721 atm

V = 4.65 L

Answer:

4.66 L of ammonia gas will be produced

Explanation:

Step 1: Data given

The pressure of ammonia gas = 547.9 mmHg = 0.72092116 atm

Temperature = 27.6 °C = 300.75 K

Mass of ammonium sulfate produced = 8.98 gramms

Molar mass of ammonium sulfate = 132.14 g/mol

Step 2: The balanced equation

2NH3(g) + H2SO4(aq) → (NH4)2SO4(s)

Step 3: Calculate moles (NH4)2SO4

Moles (NH4)2SO4 = mass (NH4)2SO4 / molar mass

Moles (NH4)2SO4 = 8.98 grams / 132.14 g/mol

Moles (NH4)2SO4 = 0.0680 moles

Step 4: Calculate moles NH3

For 1 mol (NH4)2SO4 we need 2 moles NH3

For 0.0680 moles (NH4)2SO4 we need 2*0.0680 = 0.136 moles NH3

Step 5: Calculate volume NH4

p*V=n*R*T

V = (n*R*T)/p

⇒with V = the volume of NH3 = TO BE DETERMINED

⇒with n = the number of moles NH3 = 0.136 moles NH3

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 300.75 K

⇒with p = the pressure of the gas = 0.72092116 atm

V = (0.136 * 0.08206 * 300.75) / 0.72092116

V = 4.66 L

4.66 L of ammonia gas will be produced

The question addresses the oxidation states and redox reaction balancing in chemistry, involving chromium's oxidation state in dichromate and identification of the oxidizing agent.

The question involves oxidation states and balancing redox reactions in chemistry. Regarding the oxidation state of hydrogen, it is generally +1 in compounds, not 0. For chromium in dichromate, the oxidation state is +6 (chromium(VI)), not +3. The iron half-reaction might indeed take place in acidic solution, depending on the specific reaction being discussed. The chromate half-reaction needs to have oxygen atoms balanced with water, and hydrogen atoms balanced with hydrogen ions, as indicated in the steps provided. The dichromate ion is a strong oxidizing agent, especially in acidic solution; Cr3+ does not act as the oxidizing agent in typical reactions with dichromate ions.

Answer:

The volume of carbon dioxide gas generated 468 mL.

Explanation:

The percent by mass of bicarbonate in a certain Alka-Seltzer = 32.5%

Mass of tablet = 3.45 g

Mass of bicarbonate =[tex]3.45 g\times \frac{32.5}{100}=1.121 mol[/tex]

Moles of bicarbonate ion = [tex]\frac{1.121 g/mol}{61 g/mol}=0.01840 mol[/tex]

[tex]HCO_3^{-}(aq)+HCl(aq)\rightarrow H_2O(l)+CO_2(g)+Cl^-(aq)[/tex]

According to reaction, 1 mole of bicarbonate ion gives with 1 mole of carbon dioxide gas , then 0.01840 mole of bicarbonate ion will give:

[tex]\frac{1}{1}\times 0.01840 mol=0.01840 mol[/tex] of carbon dioxide gas

Moles of carbon dioxide gas  n = 0.01840 mol

Pressure of the carbon dioxide gas = P = 1.00 atm

Temperature of the carbon dioxide gas = T = 37°C = 37+273 K=310 K

Volume of the carbon dioxide gas = V

[tex]PV=nRT[/tex] (ideal gas equation)

[tex]V=\frac{nRT}{P}=\frac{0.01840 mol\times 0.0821 atm L/mol K\times 310 K}{1.00 atm}=0.468 L[/tex]

1 L = 1000 mL

0.468 L =0.468 × 1000 mL = 468 mL

The volume of carbon dioxide gas generated 468 mL.

Final answer:

The volume of CO2 generated from a 3.45-g Alka-Seltzer tablet containing 32.5% bicarbonate is approximately 469.2 mL when reacted with stomach acid at 37°C and 1.00 atm.

Explanation:

To calculate the volume of CO2 generated from the reaction of bicarbonate (HCO^{3−}) with HCl in the stomach, we can use the provided mass percent of bicarbonate in the Alka-Seltzer tablet and the reaction stoichiometry. The balanced equation for the reaction between sodium bicarbonate and hydrochloric acid is:

NaHCO3(s) + HCl(aq) → NaCl(aq) + H2O(l) + CO2(g)

Assuming the percent by mass of bicarbonate is 32.5%, a 3.45-g tablet would contain 1.12125 g of HCO3−. The molar mass of HCO^{3−} is approximately 61 g/mol, which corresponds to 0.0184 moles of HCO^{3−}. Since the reaction produces one mole of CO2 for each mole of HCO3−, we can use the ideal gas law to calculate the volume of CO2.

At STP (0°C and 1 atm), one mole of any gas occupies 22.4 L. However, we're given conditions of 37°C and 1.00 atm. To adjust for the temperature, we can use the combined gas law:

V2 = (V1 × T2 × P1) / (T1 × P2)

Where:

Thus:

V2 = (22.4 L × 310 K) / 273 K

V2 is the volume of CO2 at the new conditions, which is approximately 25.5 L/mol. Since we have 0.0184 moles of HCO^{3−}, the volume of CO2 produced would be 0.0184 moles × 25.5 L/mol = 0.4692 L or 469.2 mL.

Answer:

Humid Continental

Marine west coast

Mediterranean

subarctic

Explanation:

just did assignment on edge

Marine west coast and Mediterranean are the types of temperate climates, due to the dispersion of precipitation throughout the year, temperate marine climates are typically distinguished by a notable lack of dry season, hence options D and E are correct.

Temperate climates are regions with moderate annual or seasonal rainfall, intermittent drought, mild to warm summers, and cool to cold winters.

Humid subtropical, marine west coast, Mediterranean are the phrases that clearly identified with temperate marine climates.

Geographically speaking, the moderate climates of Earth are found in the middle latitudes, which are halfway between the tropics and the poles.

Therefore, options D and E are correct.

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Answer:

Mass of CaCl₂ produced from the reaction = 21.31 g

Explanation:

The balanced equation for the reaction

CaCO₃(s) + 2HCl(aq) ⟶ CaCl₂(aq) + H₂O(l) + CO₂(g)

How many grams of calcium chloride will be produced when 25.0 g of calcium carbonate is combined with 14.0 g of hydrochloric acid

First of, we need to recognize the limiting reagent in this reaction.

The limiting reagent is the reagent that is totally used up in the chemical reaction; it determines the amount of other reactants that react and the amount of products that will be formed.

To know the limiting reagent, we convert the masses of the reactants given to number of moles.

Number of moles = (mass)/(molar mass)

25.0 g of calcium carbonate

Molar mass of CaCO₃ = 100.0869 g/mol

Number of moles of CaCO₃ present at the start of the reaction = (25/100.0869) = 0.250 moles

14.0 g of hydrochloric acid

Molar mass of HCl = 36.46 g/mol

Number of moles of HCl present at the start of the reaction = (14/36.45) = 0.384 moles

But from the stoichiometric balance of the reaction,

1 mole of CaCO₃ reacts with 2 moles of HCl

If CaCO₃ was the limiting reagent,

0.25 moles of CaCO₃ at the start of the reaction would require 0.50 moles of HCl; which is more than the available number of moles of HCl available at the start of the reaction (0.384 moles)

So, CaCO₃ isn't the limiting reagent.

If HCl is the limiting reagent,

0.384 moles of HCl would require 0.192 moles of CaCO₃ to react with. This is within the limit of CaCO₃ present at the start of the reaction. (0.250 moles)

Hence, HCl is the limiting reagent, it is the reactant that is used up in the reaction and determines the amount of products formed.

Again, from the stoichiometric balance of the reaction,

2 moles of HCl gives 1 mole of CaCl₂

0.384 moles of HCl will give (0.384/2) moles of CaCl₂; that is, 0.192 moles of CaCl₂

We then convert this number of moles to mass.

Mass = (number of moles) × (molar mass)

Molar mass of CaCl₂ = 110.98 g/mol

Mass of CaCl₂ produced by the reaction = 0.192 × 110.98 = 21.30816 g = 21.31 g

Hope this Helps!!!

Answer: 21.09g of Calcium chloride is produced

Explanation: Please see the attachments below

Answer:

It would evaporate.

Explanation:

If you left it on room temperature  it would evaporate.

Answer:

ph= 3.53

Explanation:

A pH of 7 is neutral. A pH less than 7 is acidic. A pH greater than 7 is basic. The pH scale is logarithmic and as a result, each whole pH value below 7 is ten times more acidic than the next higher value.

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Answer:

In the first paragraph state how climate change is the earth warming. Tell them how the warmer atmosphere has lead to the melting of snow and ice in the arctic and sever droughts in other areas of the world.

In the second paragraph talk about how large rivers are becoming smaller in regards to water volume and that the amount of water discharged into the ocean has also decreased greatly.

In the final paragraph write about how weather phenomena impact global warming. State that El Niño has led to lower floods in some place whereas other areas have experienced an increase in floods. Finally tell the reader how the lower water volumes and discharge leads to a change in the global ocean circulation.

Explanation:

Answer:

Partial pressure Kr → 546.1 mmHg

Partial pressure H₂ → 145.9 mmHg

Explanation:

To determine the partial pressure of each gas in the mixture we apply the mole fraction concept.

Mole fraction → Moles of gas / Total gas = Partial pressure / Total pressure

In this mixture: Partial pressure Kr + partial pressure H₂ = 692 mmHg

We determine the moles of each:

20.9 g / 83.80 g/mol = 0.249 moles Kr

0.133 g / 2 g/mol = 0.0665 moles H₂

Total moles: 0.249 moles Kr + 0.0665 moles H₂ = 0.3155 moles

Mole fraction Kr → 0.249 mol / 0.3155 mol = 0.789

Partial pressure Kr → 0.789 . 692mmHg = 546.1 mmHg

Partial pressure H₂ → 692mmHg - 546.1 mmHg = 145.9 mmHg

Answer : The molarity of the resulting solution is, 0.29 M

Explanation :

When NaCl dissolved in water then it dissociates to give sodium ions and chloride ions.

Given,

Moles of NaCl = 0.87 mol

Volume of solution = 3.00 L

Molarity : It is defined as the number of moles of solute present in one liter of volume of solution.

Formula used :

[tex]\text{Molarity}=\frac{\text{Moles of }NaCl}{\text{Volume of solution (in L)}}[/tex]

Now put all the given values in this formula, we get:

[tex]\text{Molarity}=\frac{0.87mol}{3.00L}=0.29mole/L=0.29M[/tex]

Therefore, the molarity of the resulting solution is, 0.29 M

In atoms, electrons exist on specific, discrete energy levels, which correspond to distinct values of the principal quantum number 'n'. Electricity fills these 'shells' from the lowest to the highest energy state. Transitions between energy levels require definite energy changes.

The energy levels of electrons in an atom can be understood using the principal quantum number often denoted by 'n'. Electrons exist only on specific, discrete energy levels and not between them. This principle is known as the quantization of energy. Each energy level is associated with a specific value of 'n', with n = 1, 2, 3, and so on. The greater the 'n' value, the higher the energy level.

Each energy level or shell can be visualized as concentric circles radiating from the nucleus of the atom. Electrons fill these shells starting from the one closest to the nucleus (lowest energy state), filling up to the one furthest from the nucleus (highest energy state). This illustrates the principle of energy states in a metal as in Figure 9.13.

Furthermore, the Bohr atom model suggests that each electron orbit around the nucleus corresponds to a distinct energy level, and each transition between these levels involves a definite energy change. Therefore, the energy levels of electrons in an atom are directly related to the amount of energy possessed by the electrons.

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Complete Question

A marine biologist is preparing a deep-sea submersible for a dive. The sub stores breathing air under high pressure in a spherical air tank that measures 74.0 wide. The biologist estimates she will need 2600 L of air for the dive. Calculate the pressure to which this volume of air must be compressed in order to fit into the air tank. Write your answer in atmospheres. Round your answer to significant digits.

Answer:

The pressure required is [tex]P_2= 12.2 \ atm[/tex]

Explanation:

Generally the volume of a sphere is mathematically denoted as

             [tex]V_s = \frac{4}{3} * \pi r^3[/tex]

Substituting [tex]r = \frac{d}{2} = \frac{74}{2} = 37cm[/tex]

          [tex]V_s = \frac{4}{3} * 3.42 * (37)^2[/tex]

               [tex]V_s = 2.121746 *10^5 cm^3[/tex]

Converting to Liters

               [tex]V_s = \frac{2.121746 *10^5}{1000}[/tex]

                [tex]V_s= 212.1746L[/tex]

Assume that the pressure at which the air is given to the diver is 1 atm when the air was occupying a volume of 2600L

So

From Charles law

               [tex]P_1V_1 = P_2 V_s[/tex]

Substituting  [tex]V_1 =2600 L[/tex] ,   [tex]P_1 = 1 atm[/tex] , [tex]V_s =212.1746L[/tex] , and making [tex]P_2[/tex] the subject we have

                 [tex]P_2 = \frac{P_1 * V_1}{V_s}[/tex]

                     [tex]= \frac{1 * 2600}{212.1746}[/tex]

                    [tex]P_2= 12.2 atm[/tex]

Answer:

We should weigh 72.1 of sodium sulfate

Explanation:

The solution must be made of sodium sulfate. This salt can be dissociated like this:

Na₂SO₄ →  2Na⁺  +  SO₄⁻²

From this dissociation we can say that, 2 moles of sodium cation are obtained from 1 mol of salt.

Therefore 0.513 moles of sodium cation will be obtained from 0.2565 moles of salt (0.513 . 1) / 2. The thing is that this number are the moles contained in 1 L of solution, and we need to prepare such 1.98 L

Molarity = mol / Volume (L) → Molarity . volume (L) = mol

0.2565 mol/L . 1.98L = 0.508 moles

These are the moles we should weigh. Let's convert them to moles:

0.508 mol . 142.06 g / 1 mol = 72.1 g

Answer:

We need 72.1 grams of Na2SO4

Explanation:

Step 1: Data given

sodium ion concentration = 0.513 mol/L

Volume = 1.98 L

Step 2: The balanced equation

Na2SO4 → 2Na+ + SO4^2-

Step 3: Calculate moles Na+

Moles Na+ = molarity Na+ * volume

Moles Na+ = 0.513 * 1.98 L

Moles Na+ = 1.01574 moles

Step 4: Calculate moles Na2SO4

For 1 mol Na2SO4 we need 2 moles Na+ and 1 mol SO4^2-

For 1.01574 moles Na+ we'll need 1.01574/2 = 0.50787 moles Na2SO4

Step 5: Calculate moles Na2SO4

Mass Na2SO4 = moles Na2SO4 * molar mass Na2SO4

Mass Na2SO4 = 0.50787 moles * 142.04 g/mol

Mass Na2SO4 = 72.1 grams

We need 72.1 grams of Na2SO4

Answer:

The volume of the oxygen gas is 0.246 L

Explanation:

Step 1: Data given

Temperature = 39 °C = 312 K

Temperature = 725 torr = 725 / 760 atm =  0.953947 atm

Mass of mercuric oxide = 3.97 grams

Molar mass of mercuric oxide = 216.59 g/mol

Step 2: The balanced equation

2HgO → 2Hg + O2

Step 3: Calculate moles mercuric oxide

Moles = mass / molar mass

Moles HgO = 3.97 grams / 216.59 g/mol

Moles HgO = 0.0183 moles

Step 3: Calculate moles oxyen

For 2 moles HgO we'll have 2 moles Hg and 1 mol O2

For 0.0183 moles HgO we'll have 0.0183/2 = 0.00915 moles O2

Step 4: Calculate volume O2

p*V = n*R*T

⇒with p = the pressure of the gas = 0.953947 atm

⇒with V = the volume of O2 gas = TO BE DETERMINED

⇒with n = the moles of O2 = 0.00915 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 312 K

V = (n*R*T)/p

V = (0.00915 moles * 0.08206 L*atm/mol*K * 312 K ) / 0.953947 atm

V = 0.246 L

The volume of the oxygen gas is 0.246 L

Final answer:

The complete thermal decomposition of 3.97 g of mercuric oxide (HgO) at 39 0C and 725 torr will produce 2.487 Liters of oxygen gas (O2). The calculations involve converting grams to moles using the molar mass of HgO, applying the stoichiometry of the decomposition reaction, and calculating the volume with the ideal gas law.

Explanation:

The question involves the chemical decomposition of mercuric oxide (HgO) to produce oxygen gas (O2) and uses the ideal gas law to calculate the volume of oxygen produced under specific conditions. To solve this problem, we'll use the ideal gas law PV=nRT along with stoichiometry.

Now, let's provide a step-by-step solution:

Therefore, 2.487 Liters of oxygen gas will be produced from the complete decomposition of 3.97 g of mercuric oxide at 39°C and 725 torr.