Question 1

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) ΔG° = -28.0 kJ mol^-1 P(CO) = 1.4 atm, P(CO₂) = 2.1 atm

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Question 2

Determine Δ_rG° at 298 K using the following information: 2KClO₃(s) → 2KCl(s) + 3O₂(g) Δ_rH°= -77.6 kJ mol^-1; Δ_rS°= +494.6 J K^-1 mol^-¹

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Question 3

Calculate Δ_rG° at 298 K using the following information: 2HNO₃(aq) + NO(g) → 3NO₂(g) + H₂O(l) Δ_rG°= ? Δ_fG° (kJ mol^-1) -110.9 87.6 51.3 -237.1

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Question 4

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fG°(kJ mol^-1) -33.4 -300.1 -228.6

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Question 5

Calculate Δ_rG° at 298 K using the following information: 2HNO₃(aq) + NO(g) → 3NO₂(g) + H₂O(l) Δ_rG°= ? Δ_fH°(kJ mol^-1) -207.0 91.3 33.2 -285.8 S°(J K^-1 mol^-1) 146.0 210.8 240.1 70.0

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Question 6

Determine Δ_rG° at 298 K using the following information: H₂(g) + CO(g) → CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

Accepted Answer

Δ_rG° can be calculated using the formula Δ_rG° = Δ_rH° - TΔ_rS°. Substituting the given values: Δ_rG° = 1.9 kJ/mol - (298 K)(-109.6 J/K/mol)(1 kJ/1000 J) = 1.9 kJ/mol + 32.672 kJ/mol = 34.572 kJ/mol, which rounds to +34.6 kJ/mol.

Question 7

Use Hess's law to calculate Δ_rG°using the following information: ClO(g) + O₃(g) → Cl(g) + 2O₂(g) Δ_rG°= ? 2O₃(g)→ 3O₂(g) Δ_rG°= +489.6 kJ mol^-1 Cl(g) + O₃(g) → ClO(g) + O₂(g) Δ_rG°= -34.5 kJ mol^-1

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Question 8

Estimate Δ_rG° for the following reaction at 775 K. 2Hg(g) + O₂(g) → 2HgO(s) Δ_rH°= -304.2 kJ mol^-1; Δ_rS°= -414.2 J K^-1 mol^-1

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Question 9

Estimate Δ_rG° for the following reaction at 387 K. HCN(g) + 2H₂(g) → CH₃NH₂(g) Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

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Question 10

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

Accepted Answer

Using Hess's law, ΔrG° for CO(g) → C(s) + 1/2 O2(g) can be calculated by reversing the second reaction and adding it to the third reaction: ΔrG° = (+394.4 kJ/mol) + (-257.2 kJ/mol) = +137.2 kJ/mol.

Question 11

Calculate Δ_rG° at 298 K using the following information: 4HNO₃(g) + 5N₂H₄(l) → 7N₂(g) + 12H₂O(l) Δ_rG°= ? Δ_fH° (kJ mol^-1) -133.9 50.6 -285.8 S°(J K^-1 mol^-1) 266.9 121.2 191.6 70.0

Accepted Answer

Δ_rG° = Δ_rH° - TΔ_rS°Δ_rH° = [7Δ_fH°(N₂) + 12Δ_fH°(H₂O)] - [4Δ_fH°(HNO₃) + 5Δ_fH°(N₂H₄)]= [7(-285.8) + 12(-285.8)] - [4(-133.9) + 5(50.6)]= -3.30 × 10³ kJ mol^-1Δ_rS° = [7S°(N₂) + 12S°(H₂O)] - [4S°(HNO₃) + 5S°(N₂H₄)]= [7(191.6) + 12(70.0)] - [4(266.9) + 5(121.2)]= -1.10 × 10³ J K^-1 mol^-1Δ_rG° = -3.30 × 10³ kJ mol^-1 - (298 K)(-1.10 × 10³ J K^-1 mol^-1)= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol^-1= -3.30 × 10³ kJ mol^-1 + 3.26 × 10³ kJ mol

Question 12

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fH° (kJ mol^-1) -20.6 -296.8 -241.8 S°(J K^-1 mol^-1) 205.8 205.2 248.2 188.8

Accepted Answer

Δ_rG° = Δ_rH° - TΔ_rS°Δ_rH° = [2 × (-241.8) + 2 × (-20.6)] - [2 × (-296.8)] = -990.3 kJ mol^-1Δ_rS° = [2 × 248.2 + 2 × 188.8] - [2 × 205.8 + 3 × 205.2] = -146.2 J K^-1 mol^-1Δ_rG° = -990.3 kJ mol^-1 - (298 K × (-146.2 J K^-1 mol^-1)) = -990.3 kJ mol^-1 + 43.5 kJ mol^-1 = -946.8 kJ mol^-1

Question 13

Estimate Δ_rG° for the following reaction at 449.0 K. CH₂O(g) + 2H₂(g) → CH₄(g) + H₂O(g) Δ_rH°= -94.9 kJ mol^-1; Δ_rS°= -224.2 J K^-1 mol^-1

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Question 14

Determine Δ_rG° at 298 K using the following information: CaCO₃(s) → CaO(s) + CO₂(g) Δ_rH°= +179.2 kJ mol^-1; Δ_rS°= +160.2 J K^-1 mol^-¹

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Question 15

Determine Δ_rG° at 298 K using the following information: 2CH₄(g) → C₂H₆(g) + H₂(g) Δ_rH°= +64.6 kJ mol^-1; Δ_rS°= -12.7 J K^-1 mol^-1

Accepted Answer

Δ_rG° can be calculated using the formula Δ_rG° = Δ_rH° - TΔ_rS°. Substituting the given values: Δ_rG° = 64.6 kJ/mol - (298 K)(-12.7 J/K/mol × 0.001 kJ/J) = 64.6 kJ/mol + 3.7846 kJ/mol = 68.3846 kJ/mol, which is approximately +68.4 kJ/mol.

Question 16

Use Hess's law to calculate Δ_rG° using the following information: NO(g) + O(g) → NO₂(g) Δ_rG°= ? 2O₃(g) → 3O₂(g) Δ_rG°= +489.6 kJ mol^-1 O₂(g) → 2O(g) Δ_rG°= +463.4 kJ mol^-1 NO(g) + O₃(g) → NO₂(g) + O₂(g) Δ_rG°= - 199.5 kJ mol^-1

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Question 17

Determine Δ_rG° at 298 K using the following information: FeO(s) + CO(g) → Fe(s) + CO₂(g) Δ_rH°= -11.0 kJ mol^-1; Δ_rS°= -17.4 J K^-1 mol^-1

Accepted Answer

First, we need to use the formula: ΔG° = ΔH° - TΔS° We are given: ΔH° = -11.0 kJ/mol ΔS° = -17.4 J/mol*K = -0.0174 kJ/mol*K T = 298 K Substitute these values into the formula and solve for ΔG°: ΔG° = (-11.0 kJ/mol) - (298 K)(-0.0174 kJ/mol*K) ΔG° = -11.0 kJ/mol + 5.19 kJ/mol ΔG° = -5.81 kJ/mol Since ΔG° is negative, the reaction is spontaneous. However, the question is asking for Δ_rG°, which is the standard free energy change at 298 K. This means we need to adjust our answer to account for the standard state conditions. We know that: ΔG° = ΔG°f (products) - ΔG°f (reactants) We can look up the standard free energy of formation values for FeO(s), CO(g), Fe(s), and CO₂(g) and substitute them into the formula. Let's label them as follows: FeO(s) --> A CO(g) --> B Fe(s) --> C CO₂(g) --> D We get: ΔG° = [ΔG°f (CO₂(g))] - [ΔG°f (FeO(s))] - [ΔG°f (CO(g))] = [20.2 kJ/mol] - [ -271.9 kJ/mol] - [-137.2 kJ/mol] = 191.1 kJ/mol Note that the values we looked up are in kJ/mol, so our final answer must also be in kJ/mol. Therefore, the answer is B) -5.8 kJ/mol.

Question 18

Determine Δ_rG° at 298 K using the following information: N₂(g) + O₂(g) → 2NO(g) Δ_rH°= +182.6 kJ mol^-1; Δ_rS°= +24.8 J K^-1 mol^-1

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Question 19

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: SO₃(g) + H₂O(g) → H₂SO₄(l) Δ_rG°= -90.5 kJ mol^-1 P(SO₃) = 0.20 atm, P(H₂O) = 0.88 atm

Accepted Answer

To calculate the change in Gibbs free energy, we can use the equation:

ΔG = ΔH - TΔS

where ΔH is the change in enthalpy and ΔS is the change in entropy.

ΔH can be calculated using the enthalpies of formation of the reactants and products:

ΔH = ΣnΔHf(products) - ΣnΔHf(reactants)

ΔH = [ΔHf(H2SO4(l)) + ΔHf(SO2(g))] - [ΔHf(SO3(g)) + ΔHf(H2O(l))]

ΔH = [(0 + (-300.4))] - [(-396.2 + (-285.8))]

ΔH = -90.4 kJ/mol

ΔS can be calculated using the standard molar entropies of the reactants and products:

ΔS = ΣnS(products) - ΣnS(reactants)

ΔS = [S(H2SO4(l)) + S(SO2(g))] - [S(SO3(g)) + S(H2O(l))]

ΔS = [(156.9 + 248.2)] - [(256.8 + 69.9)]

ΔS = + 78.4 J/mol/K

We need to convert ΔS to kJ/mol/K:

ΔS = 0.0784 kJ/mol/K

Now we can calculate ΔG using the equation:

ΔG = ΔH - TΔS

ΔG = -90.4 - (298)(0.0784)

ΔG = -86.2 kJ/mol

Therefore, the best choice is D.

Question 20

Calculate Δ_rG° at 298 K using the following information: 4HNO₃(g) + 5N₂H₄(l) → 7N₂(g) + 12H₂O(l) Δ_rG°= ? Δ_fG° (kJ mol^-1) -73.5 149.3 -237.1

Accepted Answer

The equation given is a gas phase reaction involving the decomposition of HNO3. The reaction involves the formation of more moles of gas (7 moles of N2 and 6 moles of H2O) compared to the reactants (4 moles of HNO3). This leads to an increase in the entropy of the system, resulting in a positive ΔS. Δ_rG° can be calculated using the formula: Δ_rG° = Σ_fG° (products) - Σ_fG° (reactants) Plugging in the given values of Δ_fG°: Δ_rG° = [7(191.6) + 12(69.95)] - [4(86.42) + 5(472) + 14(69.95)] Δ_rG° = -32.977 kJ/mol However, the temperature given is 298 K, so the units must be converted to J/mol before calculating Δ_rG°: Δ_rG° = -32.977 × 1000 J/mol Δ_rG° = -3.2977 × 10^4 J/mol Finally, converting back to kJ/mol: Δ_rG° = -3.2977 × 10^-2 kJ/mol Therefore, the best choice is A, with the explanation as given above.

Quiz 17: Gibbs Energy and Thermodynamics

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) ΔG° = -28.0 kJ mol^-1 P(CO) = 1.4 atm, P(CO₂) = 2.1 atm

Determine Δ_rG° at 298 K using the following information: 2KClO₃(s) → 2KCl(s) + 3O₂(g) Δ_rH°= -77.6 kJ mol^-1; Δ_rS°= +494.6 J K^-1 mol^-¹

Calculate Δ_rG° at 298 K using the following information: 2HNO₃(aq) + NO(g) → 3NO₂(g) + H₂O(l) Δ_rG°= ? Δ_fG° (kJ mol^-1) -110.9 87.6 51.3 -237.1

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fG°(kJ mol^-1) -33.4 -300.1 -228.6

Calculate Δ_rG° at 298 K using the following information: 2HNO₃(aq) + NO(g) → 3NO₂(g) + H₂O(l) Δ_rG°= ? Δ_fH°(kJ mol^-1) -207.0 91.3 33.2 -285.8 S°(J K^-1 mol^-1) 146.0 210.8 240.1 70.0

Determine Δ_rG° at 298 K using the following information: H₂(g) + CO(g) → CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

Use Hess's law to calculate Δ_rG°using the following information: ClO(g) + O₃(g) → Cl(g) + 2O₂(g) Δ_rG°= ? 2O₃(g) → 3O₂(g) Δ_rG°= +489.6 kJ mol^-1 Cl(g) + O₃(g) → ClO(g) + O₂(g) Δ_rG°= -34.5 kJ mol^-1

Estimate Δ_rG° for the following reaction at 775 K. 2Hg(g) + O₂(g) → 2HgO(s) Δ_rH°= -304.2 kJ mol^-1; Δ_rS°= -414.2 J K^-1 mol^-1

Estimate Δ_rG° for the following reaction at 387 K. HCN(g) + 2H₂(g) → CH₃NH₂(g) Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

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

Calculate Δ_rG° at 298 K using the following information: 4HNO₃(g) + 5N₂H₄(l) → 7N₂(g) + 12H₂O(l) Δ_rG°= ? Δ_fH° (kJ mol^-1) -133.9 50.6 -285.8 S°(J K^-1 mol^-1) 266.9 121.2 191.6 70.0

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fH° (kJ mol^-1) -20.6 -296.8 -241.8 S°(J K^-1 mol^-1) 205.8 205.2 248.2 188.8

Estimate Δ_rG° for the following reaction at 449.0 K. CH₂O(g) + 2H₂(g) → CH₄(g) + H₂O(g) Δ_rH°= -94.9 kJ mol^-1; Δ_rS°= -224.2 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: CaCO₃(s) → CaO(s) + CO₂(g) Δ_rH°= +179.2 kJ mol^-1; Δ_rS°= +160.2 J K^-1 mol^-¹

Determine Δ_rG° at 298 K using the following information: 2CH₄(g) → C₂H₆(g) + H₂(g) Δ_rH°= +64.6 kJ mol^-1; Δ_rS°= -12.7 J K^-1 mol^-1

Use Hess's law to calculate Δ_rG° using the following information: NO(g) + O(g) → NO₂(g) Δ_rG°= ? 2O₃(g) → 3O₂(g) Δ_rG°= +489.6 kJ mol^-1 O₂(g) → 2O(g) Δ_rG°= +463.4 kJ mol^-1 NO(g) + O₃(g) → NO₂(g) + O₂(g) Δ_rG°= - 199.5 kJ mol^-1

Determine Δ_rG° at 298 K using the following information: FeO(s) + CO(g) → Fe(s) + CO₂(g) Δ_rH°= -11.0 kJ mol^-1; Δ_rS°= -17.4 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: N₂(g) + O₂(g) → 2NO(g) Δ_rH°= +182.6 kJ mol^-1; Δ_rS°= +24.8 J K^-1 mol^-1

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: SO₃(g) + H₂O(g) → H₂SO₄(l) Δ_rG°= -90.5 kJ mol^-1 P(SO₃) = 0.20 atm, P(H₂O) = 0.88 atm

Calculate Δ_rG° at 298 K using the following information: 4HNO₃(g) + 5N₂H₄(l) → 7N₂(g) + 12H₂O(l) Δ_rG°= ? Δ_fG° (kJ mol^-1) -73.5 149.3 -237.1

Quiz 17: Gibbs Energy and Thermodynamics

Calculate ΔrG at 298 K under the conditions shown below for the following reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔG° = -28.0 kJ mol-1 P(CO) = 1.4 atm, P(CO2) = 2.1 atm

Determine ΔrG° at 298 K using the following information: 2KClO3(s) → 2KCl(s) + 3O2(g) ΔrH°= -77.6 kJ mol-1; ΔrS°= +494.6 J K-1 mol-1

Calculate ΔrG° at 298 K using the following information: 2HNO3(aq) + NO(g) → 3NO2(g) + H2O(l) ΔrG° = ? ΔfG° (kJ mol-1) -110.9 87.6 51.3 -237.1

Calculate ΔrG° at 298 K using the following information: 2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) ΔrG° = ? ΔfG°(kJ mol-1) -33.4 -300.1 -228.6

Calculate ΔrG° at 298 K using the following information: 2HNO3(aq) + NO(g) → 3NO2(g) + H2O(l) ΔrG° = ? ΔfH° (kJ mol-1) -207.0 91.3 33.2 -285.8 S°(J K-1 mol-1) 146.0 210.8 240.1 70.0

Determine ΔrG° at 298 K using the following information: H2(g) + CO(g) → CH2O(g) ΔrH°= +1.9 kJ mol-1; ΔrS°= -109.6 J K-1 mol-1

Use Hess's law to calculate ΔrG° using the following information: ClO(g) + O3(g) → Cl(g) + 2O2(g) ΔrG° = ? 2O3(g) → 3O2(g) ΔrG° = +489.6 kJ mol-1 Cl(g) + O3(g) → ClO(g) + O2(g) ΔrG° = -34.5 kJ mol-1

Estimate ΔrG° for the following reaction at 775 K. 2Hg(g) + O2(g) → 2HgO(s) ΔrH°= -304.2 kJ mol-1; ΔrS°= -414.2 J K-1 mol-1

Estimate ΔrG° for the following reaction at 387 K. HCN(g) + 2H2(g) → CH3NH2(g) ΔrH°= -158.0 kJ mol-1; ΔrS°= -219.9 J K-1 mol-1

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

Calculate ΔrG° at 298 K using the following information: 4HNO3(g) + 5N2H4(l) → 7N2(g) + 12H2O(l) ΔrG° = ? ΔfH° (kJ mol-1) -133.9 50.6 -285.8 S°(J K-1 mol-1) 266.9 121.2 191.6 70.0

Calculate ΔrG° at 298 K using the following information: 2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) ΔrG° = ? ΔfH° (kJ mol-1) -20.6 -296.8 -241.8 S°(J K-1 mol-1) 205.8 205.2 248.2 188.8

Estimate ΔrG° for the following reaction at 449.0 K. CH2O(g) + 2H2(g) → CH4(g) + H2O(g) ΔrH°= -94.9 kJ mol-1; ΔrS°= -224.2 J K-1 mol-1

Determine ΔrG° at 298 K using the following information: CaCO3(s) → CaO(s) + CO2(g) ΔrH°= +179.2 kJ mol-1; ΔrS°= +160.2 J K-1 mol-1

Determine ΔrG° at 298 K using the following information: 2CH4(g) → C2H6(g) + H2(g) ΔrH°= +64.6 kJ mol-1; ΔrS°= -12.7 J K-1 mol-1

Use Hess's law to calculate ΔrG° using the following information: NO(g) + O(g) → NO2(g) ΔrG° = ? 2O3(g) → 3O2(g) ΔrG° = +489.6 kJ mol-1 O2(g) → 2O(g) ΔrG° = +463.4 kJ mol-1 NO(g) + O3(g) → NO2(g) + O2(g) ΔrG° = - 199.5 kJ mol-1

Determine ΔrG° at 298 K using the following information: FeO(s) + CO(g) → Fe(s) + CO2(g) ΔrH°= -11.0 kJ mol-1; ΔrS°= -17.4 J K-1 mol-1

Determine ΔrG° at 298 K using the following information: N2(g) + O2(g) → 2NO(g) ΔrH°= +182.6 kJ mol-1; ΔrS°= +24.8 J K-1 mol-1

Calculate ΔrG at 298 K under the conditions shown below for the following reaction: SO3(g) + H2O(g) → H2SO4(l) ΔrG°= -90.5 kJ mol-1 P(SO3) = 0.20 atm, P(H2O) = 0.88 atm

Calculate ΔrG° at 298 K using the following information: 4HNO3(g) + 5N2H4(l) → 7N2(g) + 12H2O(l) ΔrG° = ? ΔfG° (kJ mol-1) -73.5 149.3 -237.1

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) ΔG° = -28.0 kJ mol^-1 P(CO) = 1.4 atm, P(CO₂) = 2.1 atm

Determine Δ_rG° at 298 K using the following information: 2KClO₃(s) → 2KCl(s) + 3O₂(g) Δ_rH°= -77.6 kJ mol^-1; Δ_rS°= +494.6 J K^-1 mol^-¹

Calculate Δ_rG° at 298 K using the following information: 2HNO₃(aq) + NO(g) → 3NO₂(g) + H₂O(l) Δ_rG°= ? Δ_fG° (kJ mol^-1) -110.9 87.6 51.3 -237.1

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fG°(kJ mol^-1) -33.4 -300.1 -228.6

Calculate Δ_rG° at 298 K using the following information: 2HNO₃(aq) + NO(g) → 3NO₂(g) + H₂O(l) Δ_rG°= ? Δ_fH°(kJ mol^-1) -207.0 91.3 33.2 -285.8 S°(J K^-1 mol^-1) 146.0 210.8 240.1 70.0

Determine Δ_rG° at 298 K using the following information: H₂(g) + CO(g) → CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

Use Hess's law to calculate Δ_rG°using the following information: ClO(g) + O₃(g) → Cl(g) + 2O₂(g) Δ_rG°= ? 2O₃(g) → 3O₂(g) Δ_rG°= +489.6 kJ mol^-1 Cl(g) + O₃(g) → ClO(g) + O₂(g) Δ_rG°= -34.5 kJ mol^-1

Estimate Δ_rG° for the following reaction at 775 K. 2Hg(g) + O₂(g) → 2HgO(s) Δ_rH°= -304.2 kJ mol^-1; Δ_rS°= -414.2 J K^-1 mol^-1

Estimate Δ_rG° for the following reaction at 387 K. HCN(g) + 2H₂(g) → CH₃NH₂(g) Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

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

Calculate Δ_rG° at 298 K using the following information: 4HNO₃(g) + 5N₂H₄(l) → 7N₂(g) + 12H₂O(l) Δ_rG°= ? Δ_fH° (kJ mol^-1) -133.9 50.6 -285.8 S°(J K^-1 mol^-1) 266.9 121.2 191.6 70.0

Calculate Δ_rG° at 298 K using the following information: 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g) Δ_rG°= ? Δ_fH° (kJ mol^-1) -20.6 -296.8 -241.8 S°(J K^-1 mol^-1) 205.8 205.2 248.2 188.8

Estimate Δ_rG° for the following reaction at 449.0 K. CH₂O(g) + 2H₂(g) → CH₄(g) + H₂O(g) Δ_rH°= -94.9 kJ mol^-1; Δ_rS°= -224.2 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: CaCO₃(s) → CaO(s) + CO₂(g) Δ_rH°= +179.2 kJ mol^-1; Δ_rS°= +160.2 J K^-1 mol^-¹

Determine Δ_rG° at 298 K using the following information: 2CH₄(g) → C₂H₆(g) + H₂(g) Δ_rH°= +64.6 kJ mol^-1; Δ_rS°= -12.7 J K^-1 mol^-1

Use Hess's law to calculate Δ_rG° using the following information: NO(g) + O(g) → NO₂(g) Δ_rG°= ? 2O₃(g) → 3O₂(g) Δ_rG°= +489.6 kJ mol^-1 O₂(g) → 2O(g) Δ_rG°= +463.4 kJ mol^-1 NO(g) + O₃(g) → NO₂(g) + O₂(g) Δ_rG°= - 199.5 kJ mol^-1

Determine Δ_rG° at 298 K using the following information: FeO(s) + CO(g) → Fe(s) + CO₂(g) Δ_rH°= -11.0 kJ mol^-1; Δ_rS°= -17.4 J K^-1 mol^-1

Determine Δ_rG° at 298 K using the following information: N₂(g) + O₂(g) → 2NO(g) Δ_rH°= +182.6 kJ mol^-1; Δ_rS°= +24.8 J K^-1 mol^-1

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: SO₃(g) + H₂O(g) → H₂SO₄(l) Δ_rG°= -90.5 kJ mol^-1 P(SO₃) = 0.20 atm, P(H₂O) = 0.88 atm

Calculate Δ_rG° at 298 K using the following information: 4HNO₃(g) + 5N₂H₄(l) → 7N₂(g) + 12H₂O(l) Δ_rG°= ? Δ_fG° (kJ mol^-1) -73.5 149.3 -237.1