Use the table below to answer the questions that follow: Substance ∆G (kJ/mol) C(graphite) 0 H2(g) 0 C2H2 209.2 SO2(g) -300.4 O2(g) 0 SO3(g) 370.4 CaCO3(g) -1128.8 CaO(s) -604. 17 CO2 -394.4 Calculate the ∆G for the following reactions and predict whether the reaction is spontaneous or not. Use the Gibbs free energy formation provided and this ∆Grxn= Σ∆Gproducts - Σ∆Greactants to be more specific. ______1. 2C(graphite)+ H2(g) à C2H2(g) -209.2 kJ (spontaneous) 0 kJ (equilibrium) 2 kJ (nonspontaneous) None of the above _______2. SO2(g) + 1/2O2(g) à SO3(g) -70 kJ (spontaneous) 70 kJ (nonspontaneous) 8 kJ (nonspontaneous) -670.8 kJ (spontaneous) _______3. CaCO3(g) à CaO(s) + CO2(g) 0 kJ (equilibrium) 0 kJ (spontaneous) 2 kJ (spontaneous) None of the above
Use the table below to answer the questions that follow: Substance ∆G (kJ/mol) C(graphite) 0 H2(g) 0 C2H2 209.2 SO2(g) -300.4 O2(g) 0 SO3(g) 370.4 CaCO3(g) -1128.8 CaO(s) -604. 17 CO2 -394.4 Calculate the ∆G for the following reactions and predict whether the reaction is spontaneous or not. Use the Gibbs free energy formation provided and this ∆Grxn= Σ∆Gproducts - Σ∆Greactants to be more specific. ______1. 2C(graphite)+ H2(g) à C2H2(g) -209.2 kJ (spontaneous) 0 kJ (equilibrium) 2 kJ (nonspontaneous) None of the above _______2. SO2(g) + 1/2O2(g) à SO3(g) -70 kJ (spontaneous) 70 kJ (nonspontaneous) 8 kJ (nonspontaneous) -670.8 kJ (spontaneous) _______3. CaCO3(g) à CaO(s) + CO2(g) 0 kJ (equilibrium) 0 kJ (spontaneous) 2 kJ (spontaneous) None of the above
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.14PAE: Enthalpy changes often help predict whether or not a process will be spontaneous. What type of...
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Question
Use the table below to answer the questions that follow:
Substance |
∆G (kJ/mol) |
C(graphite) |
0 |
H2(g) |
0 |
C2H2 |
209.2 |
SO2(g) |
-300.4 |
O2(g) |
0 |
SO3(g) |
370.4 |
CaCO3(g) |
-1128.8 |
CaO(s) |
-604. 17 |
CO2 |
-394.4 |
Calculate the ∆G for the following reactions and predict whether the reaction is spontaneous or not. Use the Gibbs free energy formation provided and this ∆Grxn= Σ∆Gproducts - Σ∆Greactants to be more specific.
______1. 2C(graphite)+ H2(g) à C2H2(g)
- -209.2 kJ (spontaneous)
- 0 kJ (equilibrium)
- 2 kJ (nonspontaneous)
- None of the above
_______2. SO2(g) + 1/2O2(g) à SO3(g)
- -70 kJ (spontaneous)
- 70 kJ (nonspontaneous)
- 8 kJ (nonspontaneous)
- -670.8 kJ (spontaneous)
_______3. CaCO3(g) à CaO(s) + CO2(g)
- 0 kJ (equilibrium)
- 0 kJ (spontaneous)
- 2 kJ (spontaneous)
- None of the above
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