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A mixture of 1.57 mol of N(2),1.92 mol o...

A mixture of 1.57 mol of `N_(2)`,1.92 mol of `H_(2)` and 8.17 mol of `NH_(3)` is introduced in a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant `K_(c)` for the reaction is `1.7 xx 10^(-2)`. Is the reaction at equilibrium? The reaction is `N_(2)(g)+3H_(2)(g) rarr 2NH_(3)(g)`

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To determine if the reaction is at equilibrium, we need to calculate the reaction quotient \( Q_c \) and compare it with the equilibrium constant \( K_c \). ### Step 1: Write the balanced chemical equation The balanced chemical equation for the reaction is: \[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \] ### Step 2: Calculate the concentrations of the reactants and products We will calculate the concentrations of \( N_2 \), \( H_2 \), and \( NH_3 \) using the formula: ...
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