2nd Edition

ISBN: 9780321809261

Author: John E. McMurry, Robert C. Fay

Publisher: Prentice Hall

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Textbook Question

Chapter 16.10, Problem 16.13P

Calculate ΔG for the formation of ethylene (C₂H₄) from carbon and hydrogen at 25 °C when the partial pressures are 100 atm H₂ and 0.10 atm C₂H₄.

2 C ( s ) + 2 H 2 ( g ) → C 2 H 4 ( g ) Δ G ° = 68.1 kJ

Is the reaction spontaneous in the forward or the reverse direction?

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Chapter 16.9, Problem 16.12P

Chapter 16.10, Problem 16.14CP

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Chapter 16 Solutions

General Chemistry: Atoms First

Ch. 16.1 - Predicting the Sign of S Predict the sign of S in...Ch. 16.2 - Prob. 16.2P Ch. 16.2 - Prob. 16.3CP Ch. 16.3 - Which state has the higher entropy? Explain in...Ch. 16.5 - Calculate the standard entropy of reaction at 25C...Ch. 16.6 - By determining the sign of Stotal, show whether...Ch. 16.7 - Consider the decomposition of gaseous N2O4:...Ch. 16.7 - The following data apply to the vaporization of...Ch. 16.7 - What are the signs (+, , or 0) of H, S, and G for...Ch. 16.8 - Consider the thermal decomposition of calcium...

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Calculate Δ G for the formation of ethylene (C 2 H 4 ) from carbon and hydrogen at 25 °C when the partial pressures are 100 atm H 2 and 0.10 atm C 2 H 4 . 2 C ( s ) + 2 H 2 ( g ) → C 2 H 4 ( g ) Δ G ° = 68.1 kJ Is the reaction spontaneous in the forward or the reverse direction?

Solution Summary: The author explains how free energy formation of ethylene is calculated and the direction in which the reaction is spontaneous.

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Chapter 16 Solutions