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 0.309 M HI, 4.15×10-2 M H2 and 4.15×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.46×10-2 mol of I2(g) is added to the flask? [HI] = _____M [H2] = _____ M [I2] = ____M
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 0.309 M HI, 4.15×10-2 M H2 and 4.15×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.46×10-2 mol of I2(g) is added to the flask? [HI] = _____M [H2] = _____ M [I2] = ____M
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 57QRT
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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 0.309 M HI, 4.15×10-2 M H2 and 4.15×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.46×10-2 mol of I2(g) is added to the flask?
| [HI] | = | _____M |
| [H2] | = | _____ M |
| [I2] | = | ____M |
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