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The reaction , N(2)(g) + O(2) (g) hArr 2...

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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To solve the problem, we need to determine the equilibrium concentrations of the reactants (N₂ and O₂) and the product (NO) for the reaction: \[ N_2(g) + O_2(g) \rightleftharpoons 2 NO(g) \] Given: - Initial concentration of \( [N_2] = 0.80 \, \text{mol L}^{-1} \) - Initial concentration of \( [O_2] = 0.20 \, \text{mol L}^{-1} \) - Equilibrium constant \( K_c = 1.0 \times 10^{-5} \) at 1500 K ...
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