Equilibrium partial pressures
Posted: Sat Dec 09, 2017 6:10 pm
For question 63 in chapter 11
At 25 C, K =3.2 x 10^-34 for the reaction 2 HCl(g) <-> H2(g) + Cl2(g). If a 1.0-L reaction vessel is filled with HCl at 0.22 bar, what are the equilibrium partial pressures of HCl, H2, and Cl2?
Do you have to solve this by first calculating number of moles of HCl using PV=nRT and then later converting moles of H2 and Cl2 back to pressure? Or can you just use pressure and K to solve for the partial pressures?
At 25 C, K =3.2 x 10^-34 for the reaction 2 HCl(g) <-> H2(g) + Cl2(g). If a 1.0-L reaction vessel is filled with HCl at 0.22 bar, what are the equilibrium partial pressures of HCl, H2, and Cl2?
Do you have to solve this by first calculating number of moles of HCl using PV=nRT and then later converting moles of H2 and Cl2 back to pressure? Or can you just use pressure and K to solve for the partial pressures?