Consider the reaction: H2(g) + Br2(g) --> 2HBr(g) ΔH˚ = -103.8 kJ/mol In a particular experiment, equal moles of H2(g) at 1.00atm and Br2(g) at 1.00 atm were mixed in a 1.00 L flask at 25˚C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique and 1.10 x 1013 molecules were found. For this reaction calculate the values of K, ΔG˚, and ΔS˚.
Consider the reaction: H2(g) + Br2(g) --> 2HBr(g) ΔH˚ = -103.8 kJ/mol In a particular experiment, equal moles of H2(g) at 1.00atm and Br2(g) at 1.00 atm were mixed in a 1.00 L flask at 25˚C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique and 1.10 x 1013 molecules were found. For this reaction calculate the values of K, ΔG˚, and ΔS˚.
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
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 118CP: Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal...
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Consider the reaction:
H2(g) + Br2(g) --> 2HBr(g)
ΔH˚ = -103.8 kJ/mol
In a particular experiment, equal moles of H2(g) at 1.00atm and Br2(g) at 1.00 atm were mixed in a 1.00 L flask at 25˚C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique and 1.10 x 1013 molecules were found. For this reaction calculate the values of K, ΔG˚, and ΔS˚.
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