The equilibrium constant, K, for the following reaction is 1.80 x 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 0.330 M HI, 4.42× 10-2 M H₂ and 4.42× 10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.207 mol of HI(g) is added to the flask? [HI] M [H₂] = M [12] = M Retry Entire Group 1 more group attempt remaining Submit Answer
The equilibrium constant, K, for the following reaction is 1.80 x 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 0.330 M HI, 4.42× 10-2 M H₂ and 4.42× 10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.207 mol of HI(g) is added to the flask? [HI] M [H₂] = M [12] = M Retry Entire Group 1 more group attempt remaining Submit Answer
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 101E: A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and...
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