At a particular temperature, K = 3.11 for the reaction
SO2(g)+NO2(g)=SO3(g)+NO(g)
If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of the gases.
[SO2]= ___________M
[NO2]= ___________M
[SO3]= ___________M
[NO]= ____________M
The equilibrium concentration will be calculated from the equation,
K = [SO3][NO] / [[SO2][NO2]
Let x be the change in concenration then,
equilibrium concentration of the gases would be,
[SO2] = (0.8-x)
[NO2] = (0.8-x)
[SO3] = (0.8+x)
[NO] = (0.8+x)
Feed the values,
3.11 = (0.8+x)(0.8+x)/(0.8-x)(0.8-x)
thus their is no much change at equilibrium for the gases
solving the quadratic equation for x,
x = 0.797 M
Thus, concentration of all the gases at equilibrium would be,
[SO2] = (0.8-0.797) = 0.003 M
[NO2] = (0.8-x) = 0.003 M
[SO3] = (0.8+x) = 1.597 M
[NO] = (0.8+x) = 1.597 M
Or, the answer could also be not much change in concentration at euilibrium occures. Choose the best of the two solutions.
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