I. ICE type problem The initial concentration of all the gases in the equation i

Question

I. ICE type problem The initial concentration of all the gases in the equation in a one liter container were: NO2 0.0560 M NO 0.294 M N2O 0.184 M 02 0.377 M At equilibrium the concentration of NO2-a brown gas -was measured at 0.118 M Graded Set up an ICE table to calculate the value of Ke at equilibrium Tell how you know that the equilibrium shifts left Figure all the concentration changes and amounts left at equilibrium Write a mass action expression for Ke for this reaction Substitute equilibrium concentrations and calculate a numerical value of K .

Explanation / Answer

NO2 + NO -----------> N2O + O2

Initial : 0.0560 0.294 0.184 0.377

Change : +0.062 + 0.062 - 0.062 - 0.062

Equilibrium : 0.118 0.356 0.122 0.315

The equilibrium is shifted towards left side becuase the concentration given at equilibrium is more than that at initial.

Expression of equilibirum constant,

Kc = [N2O][O2] / [NO2][NO]

Kc = 0.122 * 0.315 / ( 0.118 * 0.356 )

Kc = 0.915

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