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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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AI Generated Solution

To solve the problem, we will use the concept of equilibrium and the equilibrium constant \( K \). The reaction is given as: \[ N_2(g) + O_2(g) \rightleftharpoons 2 NO(g) \] ### Step 1: Write down the initial concentrations We are given the initial concentrations before any reaction occurs: ...
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