Question 1

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g)+ O₂(g)→ 2 HgO(s)ΔG° = -180.8 kJ P(Hg)= 0.025 atm,P(O₂)= 0.037 atm

Accepted Answer

First, we need to calculate the ΔG for the given reaction using the formula: ΔG = ΔG° + RT ln(Q) where ΔG° is the standard free energy change, R is the gas constant (8.314 J/K·mol), T is the temperature in Kelvin (298 K), and Q is the reaction quotient. Q can be calculated using the given partial pressures of Hg and O2: Q = (P(Hg))^2/ P(O₂) Q = (0.025 atm)^2/0.037 atm Q = 0.0169 atm Substituting values into the formula, we get: ΔG = -180.8 kJ + (8.314 J/K·mol × 298 K × ln(0.0169)) ΔG = -283.9 kJ/mol Finally, we can calculate the ΔG for the desired conditions using the formula: ΔG = ΔG° + RT ln(Q/P°) where P° is the standard state pressure (1 atm). For Hg and O2, we get: ΔG = -180.8 kJ + (8.314 J/K·mol × 298 K × ln(0.0169/1)^2) ΔG = -154.4 kJ/mol Therefore, the answer is B, which is the only option with a negative value. A negative ΔG indicates that the reaction is spontaneous under the given conditions.

Question 2

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. CaCO₃(s)→ CaO(s)+ CO₂(g)ΔG° =+131.1 kJ P(CO₂)= 0.033 atm

Accepted Answer

To calculate ΔG under non-standard conditions, use the formula ΔG = ΔG° + RTlnQ, where Q is the reaction quotient. For the given reaction, Q = P(CO2), since it's the only gaseous product. At 298 K, R = 8.314 J/(mol·K) (or 0.008314 kJ/(mol·K) for consistency with ΔG° units). Thus, ΔG = 131.1 kJ + (0.008314 kJ/(mol·K) * 298 K * ln(0.033)). Calculating this gives a ΔG close to +122.6 kJ, indicating that the reaction is less spontaneous under the given conditions than under standard conditions, but still not spontaneous.

Question 3

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g)+ 5 N₂H₄(l)→ 7 N₂(g)+ 12 H₂O(l)ΔG°_rxn= ? ΔG°_f (kJ/mol)-73.5 149.3 -237.1

Accepted Answer

The answer of Calculate the ΔG°_rxn using the following information....

Question 4

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 3 O₂(g)→ 2 O₃(g)ΔG° = +326 kJ P(O₂)= 0.41 atm,P(O₃)= 5.2 atm

Accepted Answer

The answer of Calculate ΔG_rxn at 298 K under the...

Question 5

What can change the direction of a reversible reaction?

Accepted Answer

Changes in temperature, pressure, and volume can all affect the position of equilibrium for a reversible reaction. Increasing the temperature shifts the equilibrium to the endothermic direction, while decreasing it shifts it towards the exothermic direction. Increasing pressure or decreasing volume shifts the equilibrium towards the side with fewer moles of gas, while decreasing pressure or increasing volume shifts it towards the side with more moles of gas. Therefore, all of these factors can change the direction of a reversible reaction, and the best choice is D.

Question 6

Use Hess's law to calculate ΔG°_rxn using the following information. CO(g)→ C(s)+ 1/2 O₂(g)ΔG°_rxn= ? CO₂(g)→ C(s)+ O₂(g)ΔG°_rxn= +394.4 kJ CO(g)+ 1/2 O₂(g)→ CO₂(g)ΔG°_rxn= -257.2 kJ

Accepted Answer

The answer of Use Hess's law to calculate ΔG°_rxn using...

Question 7

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g)+ O(g)→ NO₂(g)ΔG°_rxn= ? 2 O₃(g)→ 3 O₂(g)ΔG°_rxn= +489.6 kJ O₂(g)→ 2 O(g)ΔG°_rxn= +463.4 kJ NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)ΔG°_rxn= - 199.5 kJ

Accepted Answer

We can use Hess's law to calculate the overall ΔG°_rxn by summing the ΔG°_rxn values for each step in the reaction: 1. NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔG°_rxn= -199.5 kJ (given) 2. O₂(g) → 2 O(g) ΔG°_rxn= +463.4 kJ (given) 3. 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ (given, but reversed in order to match reaction 1) Adding these three reactions and their respective ΔG°_rxn values gives: NO(g) + 2O₃(g) → NO₂(g) + 3O(g) ΔG°_rxn= -199.5 kJ + (+463.4 kJ) + (-489.6 kJ) ΔG°_rxn= -225.7 kJ Therefore, the best answer choice is C, -676.0 kJ. However, this answer is not provided in the choices, so the closest choice is A, +753.5 kJ, which is the reverse of the correct answer.

Question 8

Choose the statement below that is TRUE.

Accepted Answer

The answer of Choose the statement below that is TRUE.
...

Question 9

Give the name of the reaction that does not achieve the theoretical limits with respect to free energy in thermodynamics.

Accepted Answer

An irreversible reaction does not achieve the theoretical limits with respect to free energy in thermodynamics because it has a much lower efficiency compared to a reversible reaction, where free energy is conserved. In an irreversible reaction, there is a loss of free energy due to the dissipation of energy into the surroundings.

Question 10

Use Hess's law to calculate ΔG°_rxn using the following information. ClO(g)+ O₃(g)→ Cl(g)+ 2 O₂(g)ΔG°_rxn= ? 2 O₃(g)→ 3 O₂(g)ΔG°_rxn= +489.6 kJ Cl(g)+ O₃(g)→ ClO(g)+ O₂(g)ΔG°_rxn= -34.5 kJ

Accepted Answer

The answer of Use Hess's law to calculate ΔG°_rxn using...

Question 11

Which of the following is NOT true for ΔG_rxn?

Accepted Answer

The answer of Which of the following is NOT true...

Question 12

Below what temperature does the following reaction become nonspontaneous? 2 HNO₃(aq)+ NO(g)→ 3 NO₂(g)+ H₂O(l)ΔH = +136.5 kJ; ΔS = +287.5 J/K

Accepted Answer

The answer of Below what temperature does the following reaction...

Question 13

Determine ΔG°_rxn using the following information. 2 H₂S(g)+ 3 O₂(g)→ 2 H₂O(l)+ 2 SO₂(g)ΔH°= +1.12 kJ; ΔS°= -390.7 J/K

Accepted Answer

The answer of Determine ΔG°_rxn using the following information. 2...

Question 14

Determine ΔG°_rxn using the following information. H₂(g)+ CO(g)→ CH₂O(g)ΔH°= +1.9 kJ; ΔS°= -109.6 J/K

Accepted Answer

The answer of Determine ΔG°_rxn using the following information. H₂(g)+...

Question 15

Calculate the ΔG°_rxn using the following information. 2 H₂S(g)+ 3 O₂(g)→ 2 SO₂(g)+ 2 H₂O(g)ΔG°_rxn= ? ΔH°_f (kJ/mol)-20.6 -296.8 -241.8 S°(J/mol^∙K)205.8 205.2 248.2 188.8

Accepted Answer

The correct answer is A because the ΔG°_rxn can be calculated using the equation ΔG°_rxn = ΣΔG°_f(products) - ΣΔG°_f(reactants). Plugging in the values from the table, we get ΔG°_rxn = [2ΔG°_f(SO₂) + 2ΔG°_f(H₂O)] - [2ΔG°_f(H₂S) + 3ΔG°_f(O₂)] = [2(-241.8 kJ/mol) + 2(-228.6 kJ/mol)] - [2(-20.6 kJ/mol) + 3(0 kJ/mol)] = -990.3 kJ.

Question 16

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq)+ NO(g)→ 3 NO₂(g)+ H₂O(l)ΔG°_rxn= ? ΔG°_f (kJ/mol)-110.9 87.6 51.3 -237.1

Accepted Answer

The answer of Calculate the ΔG°_rxn using the following information....

Question 17

Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics.

Accepted Answer

A reversible reaction is the only type of reaction that can achieve the theoretical limits with respect to free energy in thermodynamics. This is because a reversible reaction can reach a state of equilibrium, where the forward and reverse reactions are occurring at equal rates, and the free energy of the system is at a minimum. In contrast, irreversible reactions result in a loss of free energy to the surroundings, while nonspontaneous reactions require an input of free energy to occur.

Question 18

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq)+ NO(g)→ 3 NO₂(g)+ H₂O(l)ΔG°_rxn= ? ΔH°_f (kJ/mol)-207.0 91.3 33.2 -285.8 S°(J/mol^∙K 146.0 210.8 240.1 70.0

Accepted Answer

The answer of Calculate the ΔG°_rxn using the following information....

Question 19

Given the following equation, N₂O(g)+ NO₂(g)→ 3 NO(g)ΔG°_rxn = -23.0 kJ Calculate ΔG°_rxn for the following reaction. 3 NO(g)→ N₂O(g)+ NO₂(g)

Accepted Answer

The ΔG° for the reverse reaction is the negative of the ΔG° for the forward reaction, making the correct answer 23.0 kJ.

Question 20

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g)+ 5 N₂H₄(l)→ 7 N₂(g)+ 12 H₂O(l)ΔG°_rxn= ? ΔH°_f (kJ/mol)-133.9 50.6 -285.8 S°(J/mol^∙K)266.9 121.2 191.6 70.0

Accepted Answer

ΔG°_rxn = ΔH°_rxn - TΔS°_rxnΔH°_rxn = [7(-0) + 12(-285.8)] - [4(-133.9) + 5(50.6)] = -3.30 × 10³ kJΔS°_rxn = [7(191.6) + 12(70.0)] - [4(266.9) + 5(121.2)] = -112.6 J/mol^∙KΔG°_rxn = -3.30 × 10³ kJ - (298 K)(-112.6 J/mol^∙K) = -3.30 × 10³ kJ

Quiz 19: Free Energy and Thermodynamics

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O₂) = 0.037 atm

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. CaCO₃(s) → CaO(s) + CO₂(g) ΔG° =+131.1 kJ P(CO₂) = 0.033 atm

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -73.5 149.3 -237.1

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 3 O₂(g) → 2 O₃(g) ΔG° = +326 kJ P(O₂) = 0.41 atm,P(O₃) = 5.2 atm

What can change the direction of a reversible reaction?

Use Hess's law to calculate ΔG°_rxn using the following information. CO(g) → C(s) + 1/2 O₂(g) ΔG°_rxn= ? CO₂(g) → C(s) + O₂(g) ΔG°_rxn= +394.4 kJ CO(g) + 1/2 O₂(g) → CO₂(g) ΔG°_rxn= -257.2 kJ

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g) + O(g) → NO₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ O₂(g) → 2 O(g) ΔG°_rxn= +463.4 kJ NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔG°_rxn= - 199.5 kJ

Choose the statement below that is TRUE.

Give the name of the reaction that does not achieve the theoretical limits with respect to free energy in thermodynamics.

Use Hess's law to calculate ΔG°_rxn using the following information. ClO(g) + O₃(g) → Cl(g) + 2 O₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ Cl(g) + O₃(g) → ClO(g) + O₂(g) ΔG°_rxn= -34.5 kJ

Which of the following is NOT true for ΔG_rxn?

Below what temperature does the following reaction become nonspontaneous? 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔH = +136.5 kJ; ΔS = +287.5 J/K

Determine ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 H₂O(l) + 2 SO₂(g) ΔH°= +1.12 kJ; ΔS°= -390.7 J/K

Determine ΔG°_rxn using the following information. H₂(g) + CO(g) → CH₂O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔH°_f (kJ/mol) -20.6 -296.8 -241.8 S°(J/mol^∙K) 205.8 205.2 248.2 188.8

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -110.9 87.6 51.3 -237.1

Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics.

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol^∙K 146.0 210.8 240.1 70.0

Given the following equation, N₂O(g) + NO₂(g) → 3 NO(g) ΔG°_rxn = -23.0 kJ Calculate ΔG°_rxn for the following reaction. 3 NO(g) → N₂O(g) + NO₂(g)

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol^∙K) 266.9 121.2 191.6 70.0

Quiz 19: Free Energy and Thermodynamics

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O2) = 0.037 atm

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. CaCO3(s) → CaO(s) + CO2(g) ΔG° =+131.1 kJ P(CO2) = 0.033 atm

Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -73.5 149.3 -237.1

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.41 atm,P(O3) = 5.2 atm

What can change the direction of a reversible reaction?

Use Hess's law to calculate ΔG°rxn using the following information. CO(g) → C(s) + 1/2 O2(g) ΔG°rxn = ? CO2(g) → C(s) + O2(g) ΔG°rxn = +394.4 kJ CO(g) + 1/2 O2(g) → CO2(g) ΔG°rxn = -257.2 kJ

Use Hess's law to calculate ΔG°rxn using the following information. NO(g) + O(g) → NO2(g) ΔG°rxn = ? 2 O3(g) → 3 O2(g) ΔG°rxn = +489.6 kJ O2(g) → 2 O(g) ΔG°rxn = +463.4 kJ NO(g) + O3(g) → NO2(g) + O2(g) ΔG°rxn = - 199.5 kJ

Choose the statement below that is TRUE.

Give the name of the reaction that does not achieve the theoretical limits with respect to free energy in thermodynamics.

Use Hess's law to calculate ΔG°rxn using the following information. ClO(g) + O3(g) → Cl(g) + 2 O2(g) ΔG°rxn = ? 2 O3(g) → 3 O2(g) ΔG°rxn = +489.6 kJ Cl(g) + O3(g) → ClO(g) + O2(g) ΔG°rxn = -34.5 kJ

Which of the following is NOT true for ΔGrxn?

Below what temperature does the following reaction become nonspontaneous? 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔH = +136.5 kJ; ΔS = +287.5 J/K

Determine ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔH°= +1.12 kJ; ΔS°= -390.7 J/K

Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K

Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔG°rxn = ? ΔH°f (kJ/mol) -20.6 -296.8 -241.8 S°(J/mol∙K) 205.8 205.2 248.2 188.8

Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1

Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics.

Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 3 NO(g) → N2O(g) + NO2(g)

Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol∙K) 266.9 121.2 191.6 70.0

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O₂) = 0.037 atm

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. CaCO₃(s) → CaO(s) + CO₂(g) ΔG° =+131.1 kJ P(CO₂) = 0.033 atm

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -73.5 149.3 -237.1

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 3 O₂(g) → 2 O₃(g) ΔG° = +326 kJ P(O₂) = 0.41 atm,P(O₃) = 5.2 atm

Use Hess's law to calculate ΔG°_rxn using the following information. CO(g) → C(s) + 1/2 O₂(g) ΔG°_rxn= ? CO₂(g) → C(s) + O₂(g) ΔG°_rxn= +394.4 kJ CO(g) + 1/2 O₂(g) → CO₂(g) ΔG°_rxn= -257.2 kJ

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g) + O(g) → NO₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ O₂(g) → 2 O(g) ΔG°_rxn= +463.4 kJ NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔG°_rxn= - 199.5 kJ

Use Hess's law to calculate ΔG°_rxn using the following information. ClO(g) + O₃(g) → Cl(g) + 2 O₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ Cl(g) + O₃(g) → ClO(g) + O₂(g) ΔG°_rxn= -34.5 kJ

Which of the following is NOT true for ΔG_rxn?

Below what temperature does the following reaction become nonspontaneous? 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔH = +136.5 kJ; ΔS = +287.5 J/K

Determine ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 H₂O(l) + 2 SO₂(g) ΔH°= +1.12 kJ; ΔS°= -390.7 J/K

Determine ΔG°_rxn using the following information. H₂(g) + CO(g) → CH₂O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔH°_f (kJ/mol) -20.6 -296.8 -241.8 S°(J/mol^∙K) 205.8 205.2 248.2 188.8

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -110.9 87.6 51.3 -237.1

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol^∙K 146.0 210.8 240.1 70.0

Given the following equation, N₂O(g) + NO₂(g) → 3 NO(g) ΔG°_rxn = -23.0 kJ Calculate ΔG°_rxn for the following reaction. 3 NO(g) → N₂O(g) + NO₂(g)

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol^∙K) 266.9 121.2 191.6 70.0