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11 Dec 2019
The equilibrium constant, K, for the following reaction is 1.80Ã10-2 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 0.322 M HI, 4.33Ã10-2 M H2 and 4.33Ã10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.213 mol of HI(g) is added to the flask?
[HI] = M [H2] = M [I2] = M
The equilibrium constant, K, for the following reaction is 1.80Ã10-2 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 0.322 M HI, 4.33Ã10-2 M H2 and 4.33Ã10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.213 mol of HI(g) is added to the flask?
[HI] | = | M |
[H2] | = | M |
[I2] | = | M |
Nestor RutherfordLv2
13 Dec 2019