It's tough to do these pressure problems with a computer. So you will know that p(H2) will mean pressure of H2 gas, etc.
CO(g) + 2 H2(g) ⇌ CH3OH(g)
Kp = p(CH3OH)/p(CO)*p(H2)^2
Kp = 490/[0.272*(0.608)^2] = ?
For the equilibrium:
CO(g) + 2 H2(g) ⇌ CH3OH(g)
Calculate the value of Kp given these equilibrium partial pressures: carbon monoxide, 0.272 atm; hydrogen, 0.608 atm; methanol,0.490 atm.
I am unsure of how to calculate the equation to get the answer
3 answers
4.87?
That looks OK to me. Note the I made a typo; i.e., the 490 should read 0.490. You used the correct value.