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The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K.

 

An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.325 M HI, 4.36×10-2 M H2, and 4.36×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.244 mol of HI(g) is added to the flask?

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Related questions

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 0.304 M HI, 4.07×10-2 M H2 and 4.07×10-2 M I2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.26×10-2 mol of I2(g) is added to the flask?

[HI] = M

[H2] = M

[I2] = M

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For the reaction H2(g) + I2(g) 2 HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.056 g H2 and 4.36 g I2. What is the mass of HI in the flask?

The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.321 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [I2] = M

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