the following reaction has a Kp = 109 at 25 degrees C
2NO(g) + Br2(g) reversible 2NOBr(g)
If the equilibrium partial pressure of Br2 is 0.0159 atm and equil pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equlibrium.
What are the steps to follow for this problem?
To calculate the partial pressure of NO at equilibrium, you can use the given equilibrium constant (Kp) and the partial pressures of Br2 and NOBr. The steps to follow for this problem are as follows:
1. Write the balanced chemical equation for the reaction: 2NO(g) + Br2(g) ⇌ 2NOBr(g)
2. Determine the expression for the equilibrium constant (Kp) using the coefficients from the balanced equation and the stoichiometric coefficients. In this case, the expression is: Kp = (P(NOBr)^2) / (P(NO)^2 * P(Br2))
3. Substitute the given values into the equilibrium constant expression. We have Kp = 109, P(Br2) = 0.0159 atm, and P(NOBr) = 0.0768 atm.
4. Rearrange the expression to solve for the unknown pressure, P(NO). In this case, P(NO) is the only unknown.
5. Substitute the given values into the rearranged expression and solve for P(NO).