Question

nitrogen monoxide and water react to form ammonia and oxygen, like this: 4no(g)+6h₂o(g)→4nh₃(g)+5o₂(g) write the pressure equilibrium constant expression for this reaction.

Explanation:

Step1: Recall the formula for pressure equilibrium constant

For a general reaction \(aA(g)+bB(g)
ightleftharpoons cC(g)+dD(g)\), the pressure equilibrium constant \(K_p=\frac{P_C^c\times P_D^d}{P_A^a\times P_B^b}\), where \(P\) represents partial pressure and \(a,b,c,d\) are stoichiometric coefficients.

Step2: Identify reactants and products and their stoichiometric coefficients

In the reaction \(4NO(g)+6H_2O(g)\to4NH_3(g)+5O_2(g)\), the reactants are \(NO\) (coefficient \(a = 4\)) and \(H_2O\) (coefficient \(b=6\)), and the products are \(NH_3\) (coefficient \(c = 4\)) and \(O_2\) (coefficient \(d = 5\)).

Step3: Substitute into the formula

Substituting the values into \(K_p=\frac{P_{products}}{P_{reactants}}\) (with exponents as stoichiometric coefficients), we get \(K_p=\frac{P_{NH_3}^4\times P_{O_2}^5}{P_{NO}^4\times P_{H_2O}^6}\)

Answer:

\(K_p=\frac{P_{NH_3}^4\times P_{O_2}^5}{P_{NO}^4\times P_{H_2O}^6}\)