Given is the reaction: CH4(g) + 2O2 (g) → CO2(g) + 2H2O (g) ΔG°f CH4 = -50.5 KJ/mol ΔG°f H2O = -288.6 KJ/mol ΔG°f CO2 = -394.4 KJ/mol ΔG°f O2 = 0 Calculate ΔG at 200 °C for this reaction where methane gas at 3.0 atm and oxygen gas at 7.0 atm are converted to CO2 and water both in gaseous state at 3 atm and 5 atm respectively 1. Calculate what is the ΔG° = 2. Calculate the value of Q = 3. Calculate the ΔG = Answer Format: 2 decimal places in scientific notation no space in between characters (ex. 1.11x10^-2)
Given is the reaction: CH4(g) + 2O2 (g) → CO2(g) + 2H2O (g) ΔG°f CH4 = -50.5 KJ/mol ΔG°f H2O = -288.6 KJ/mol ΔG°f CO2 = -394.4 KJ/mol ΔG°f O2 = 0 Calculate ΔG at 200 °C for this reaction where methane gas at 3.0 atm and oxygen gas at 7.0 atm are converted to CO2 and water both in gaseous state at 3 atm and 5 atm respectively 1. Calculate what is the ΔG° = 2. Calculate the value of Q = 3. Calculate the ΔG = Answer Format: 2 decimal places in scientific notation no space in between characters (ex. 1.11x10^-2)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter16: Spontaneity Of Reaction
Section: Chapter Questions
Problem 83QAP
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Given is the reaction:
CH4(g) + 2O2 (g) → CO2(g) + 2H2O (g)
ΔG°f CH4 = -50.5 KJ/mol
ΔG°f H2O = -288.6 KJ/mol
ΔG°f CO2 = -394.4 KJ/mol
ΔG°f O2 = 0
Calculate ΔG at 200 °C for this reaction where methane gas at 3.0 atm and oxygen gas at 7.0 atm are converted to CO2 and water both in gaseous state at 3 atm and 5 atm respectively
1. Calculate what is the ΔG° =
2. Calculate the value of Q =
3. Calculate the ΔG =
Answer Format: 2 decimal places in scientific notation no space in between characters (ex. 1.11x10^-2)
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