The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K.2HI (g) H2 (g) + I2 (g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.326 M HI, 4.38×10-2 M H2 and 4.38×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.43×10-2 mol of H2(g) is added to the flask?
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K.2HI (g) H2 (g) + I2 (g) An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.326 M HI, 4.38×10-2 M H2 and 4.38×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.43×10-2 mol of H2(g) is added to the flask?
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K.
2HI
- (g)
H2
- (g) +
I2
- (g)
An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.326 M HI, 4.38×10-2 M H2 and 4.38×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.43×10-2 mol of H2(g) is added to the flask?
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