In: Chemistry
For the following reaction, Keq is 0.00183 at 390. K: PCl5(g) PCl3(g) + Cl2(g) If 2.89 g of PCl5 is placed in a 2.86 L bulb at 390. K, what is the equilibrium pressure of Cl2? 1 atm = 1.013 bar
answer in bar
PCl5(g)------------> PCl3(g) + Cl2(g)
no of moles of PCl5 = W/G.M.Wt
= 2.89/208 = 0.0139moles
PV = nRT
P = nRT/V
= 0.0139*0.0821*390/2.86 = 0.156atm
PCl5(g) ---------->PCl3(g) + Cl2(g)
I 0.156 0 0
C -x +x +x
E 0.156-x +x +x
Kp = PPCl3 PCl2/PPCl5
0.00183 = x*x/0.156-x
0.00183*(0.156-x) = x2
x = 0.016
PXl2 = x = 0.016atm = 0.016*1.013 = 0.016208bar