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A mixture of 3.00 mol of Cl2 and 3.00 mol of CÓ is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed. CO(g) + Cl2 (g)= COC2 (g) a. Calculate K, for the reaction at 600.°C. K. b. Calculate AG° for the reaction at this temperature. AG° : kJ/mol

A mixture of 3.00 mol of Cl2 and 3.00 mol of CÓ is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed. CO(g) + Cl2 (g)= COC2 (g) a. Calculate K, for the reaction at 600.°C. K. b. Calculate AG° for the reaction at this temperature. AG° : kJ/mol

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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A mixture of 3.00 mol of Cl2 and 3.00 mol of CO is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed.

A) Calculate  for the reaction at 600.°C. 

B) Calculate for ΔG° the reaction at this temperature.

A mixture of 3.00 mol of Cl2 and 3.00 mol of CÓ is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed. CO(g) + Cl2 (g)= COC2 (g) a. Calculate K, for the reaction at 600.°C. K. b. Calculate AG° for the reaction at this temperature. AG° : kJ/mol
Transcribed Image Text:A mixture of 3.00 mol of Cl2 and 3.00 mol of CÓ is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed. CO(g) + Cl2 (g)= COC2 (g) a. Calculate K, for the reaction at 600.°C. K. b. Calculate AG° for the reaction at this temperature. AG° : kJ/mol
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