‘At 600.0 K, the equilibrium constant based on pressure is Kp = 1.83 x 10^2. Gaseous C2H4 and H2O are placed in a 1.2 L closed flask at 600.0 K. At equilibrium, the flask contains 0.0062 mol of C2H4 and 0.041 mol of H2O. Determine the equilibrium constant Kc assuming the pressure of the gases is in atmospheres.’

Question

I know the relationship between Kp and Kc, but how do I determine the value of delta n? Do I find the limiting reagent to calculate the moles of C2H5OH and then use that?

Thanks!

Answer 1

Also, how would I find the partial pressure of C2H5OH if I don't know the number of moles there are?

Thanks so much, I feel like I half-understand these and then I don't.