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InterviewSolution
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The reaction , `N_(2)(g) + O_(2) (g) hArr 2 NO(g)` contribute to air pollution whenever a fuel is burnt in air at a high temperature . At 1500 K , quilibrium constant K for its is `1.0 xx 10^(-5)` . Suppose in a case `[N_(2)] = 0.80 mol L^(-1)` and `[O_(2)] = 0.20 mol L^(-1)` before any reaction occurs . Calculate the equilibrium concentrations of the reactants and the product after the mixture has been heated to 1500 K. |
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Answer» `N_(2)(g) + O_(2)(g) hArr 2NO(g) T = 1500 K K = 1.0 xx 10^(-5)` `{:([N_(2)]_(i) = 0.80 M [O_(2)] = 0.20 M " "N_(2) " "+ " "O_(2)hArr 2NO) , (t = O " "a " " b " "O), (t=t " "a-x " " b-x " "ax):}` `K = ([2x]^(2))/((a-x) (b-x))` `1.0 xx 10^(-5) = (4x^(2))/((0.80-x)(0.20 -x))` `4 xx 105 x^(2) + x - 0.16 = 0` Using quardratic formula `x = + 6.3 xx 10^(-4)` `therefore " "` [No]= `2x = 1.26 xx 10^(-3)M` `[N_(2)] = 0.80 - 6.3 xx 10^(-4) = 0.799M` `[O_(2)] = 0.20 - 6.3 xx 10^(-4) = 0.199 M` |
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