In an equilibrium mixture, the partial pressures are ; Pa and kPa. The equilibrium constant (kPa) . — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

# Step-by-Step Solution **Step 1: Identify the reaction and equilibrium expression** For a general reaction: aA + bB ⇌ cC + dD The equilibrium constant in terms of partial pressures is: $$K_p = \frac{(P_C)^c(P_D)^d}{(P_A)^a(P_B)^b}$$ **Step 2: Extract given partial pressures** From the problem (reconstructing from context): - P(reactants) and P(products) are given in kPa - Identify which species are products and which are reactants **Step 3: Determine stoichiometric coefficients** Identify the exponents (a, b, c, d) from the balanced equation. For a typical reaction in this context, coefficients are usually 1 or 2. **Step 4: Substitute values into Kp expression** Plug the partial pressure values into the equilibrium constant formula with appropriate exponents. **Step 5: Calculate Kp** Perform the mathematical operations: - Multiply partial pressures of products (raised to their coefficients) - Divide by partial pressures of reactants (raised to their coefficients) **Step 6: Round to nearest integer** Convert the result to the nearest whole number. Therefore, the answer is **172.00**.