For the reaction: 2NO(g) + H2(g) <=> N2O(g) + H2O(g) + energy
Write the equilibrium constant expression for the reaction.
This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of H2 is 3.00 mol/L, the concentration of N2O is 4.00 mol/L, and the concentration of H2O is 1.25 mol/L. Using the balanced chemical equation, calculate the equilibrium constant for this system.
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To write the equilibrium constant expression for the reaction, we need to use the concentrations of the reactants and products in the balanced chemical equation.
The equilibrium constant expression is given by:
Kc = ([N2O] * [H2O]) / ([NO]^2 * [H2])
Using the concentrations given:
[N2O] = 4.00 mol/L
[H2O] = 1.25 mol/L
[NO] = 1.75 mol/L
[H2] = 3.00 mol/L
Substituting these values into the equilibrium constant expression:
Kc = (4.00 * 1.25) / (1.75^2 * 3.00)
Now we can calculate the equilibrium constant value using a calculator.
Kc = (4.00 * 1.25) / (1.75^2 * 3.00) = 0.380
Therefore, the equilibrium constant for this system is approximately 0.380.