For the following reaction: 2CH4(g) + O2(g) → 2CO(g) + 4H2(g) Compound ΔH°f (kJ mol-1)...
For the following reaction:
2CH4(g) + O2(g) → 2CO(g) +
4H2(g)
| Compound | ΔH°f (kJ mol-1) | S° (J mol-1 K-1) | ||
| CH4 (g) | -74.87 | 188.66 | ||
| O2 (g) | 0.00 | 205.70 | ||
| CO (g) | -110.53 | 197.66 | ||
| H2 (g) | 0.00 | 130.68 |
Calculate ΔG°rx (in kJ) at 345.31 K for this reaction.
Report your answer to two decimal places in standard notation
(i.e. 123.45 kJ).
Assume ΔH°f and S° do not vary as a function of
temperature.
Homework Answers
Your answer is -187.05 KJ
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For the following reaction:
2CH4(g) + O2(g) → 2CO(g) +
4H2(g)
Compound
ΔH°f (kJ mol-1)...
For the following reaction: CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) Compound ΔH°f (kJ mol-1)...
For the following reaction: CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CS2 (g) 116.70 237.80 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 SO2 (g) -296.84 248.20 Calculate ΔG°rx (in kJ) at 794.8 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and S° do not vary as a function of temperature.
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From the enthalpies of reaction 2C(s)+O2(g)→2CO(g)ΔH=−221.0kJ 2C(s)+O2(g)+4H2(g)→2CH3OH(g)ΔH=−402.4kJ calculate Δ...
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If the ΔH°rx and ΔS°rx for a gas phase chemical reaction are 419.53 kJ and -178.85...
If the ΔH°rx and ΔS°rx for a gas phase chemical reaction are 419.53 kJ and -178.85 J/K respectively, determine ΔG°rx (in kJ) at 103.11 °C. Report your answer to two decimal places (i.e. 123.45 kJ). Assume that ΔH°rx and ΔS°rx do not vary with temperature.
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calculate the value for the thermodynamic equilibrium constant for the following reaction. CS2 (g) + 4H2...
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