I am trying to solve the equilibrium concentration by solving for X, I understan

Question

I am trying to solve the equilibrium concentration by solving for X, I understand setting up all of the equation up until this point

Consider the following reaction:2 H2O(g) + 2 SO2(g) ?2 H2S(g) + 3 O2(g). A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kcfor the reaction at this temperature is 1.3 × 10-6

How am I supposed to solve for an interger exponent? Quadradic equation?

Explanation / Answer

your ICE table is correct

I am continuing according to ICE table

Kc = [H2S]^2[O2]^3/[H2O]^2[SO2]^2

1.3*10^-6 = (2x)*(3x)/(2.8-2x)(2.6-2x)

9.5*10^-6 - 1.4*10^-5x + 5.2*10^-6 X^2 = 6x^2
omit the 5.2*10^-6 X^2 value since 6x^2 is very large

6x^2 + 1.4*10^-5x - 9.5*10^-6 = 0

by solving the above quadratic equation

x = 1.26*10^-3

[H2S] = 2x = 2*1.26*10^-3 = 2.52*10^-3 M

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