Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 °C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm.

Question

Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 °C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm.

H2(g)+I2(g) = 2HI(g)

is it like this, (5.462)^2/(0.2282x0.1646)

Answer 1

Yes, but to keep from making a mistake in the future I would place parentheses around BOTH of the reactants, as this.

(5.462)^2/((0.2282)(0.1636).
You may come across something in the future in which one of them is squared and the other is not and you don't want to get in the habit of placing them together as you did here. What you did, however, is not incorrect.