1.30 mol each of CO} and Cl2 are introduced into an evacuated 1.80 L flask, and the following equilibrium is established at 668 K.
CO + Cl2 +++> COCl2 kp = 22.5
Calculate partial pressure of COCl2. i get about 30.9. but its wrong. i solved for x, COCL2/CO*Cl2, using ICE formula, converted everything to molarity, then to moles, then using ideal gas law. still cant get it.
If I work this I don't get 30.9 but 38.28 atm. I wonder why you converted to molarity since Kp is given and they want the answer in partial pressure COCl2?
I used PV = nRT. Plug in the numbers and obtain PCO and PCl2. Something like 39.6 atm or so. Then set up the ICE chart using atm and it becomes
x/(39.6-x)^2 = 22.5 and solve for x.
1.30 mol each of CO} and Cl2 are introduced into an evacuated 1.80 L flask, and the following equilibrium is established at 668 K. CO + Cl2 +++> COCl2 kp = 22.5 Calculate partial pressure of COCl2. i get about 30.9. but its wrong.
At 35°C, K = 1.6 10-5 mol/L for the following reaction. 2 NOCl(g) 2 NO(g) + Cl2(g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. (a) 3.8 mol of pure NOCl in a 2.0-L flask
K=1.6x10^-5 mol/L for the following reaction 2NOCl(g).... 2 NO(g) + Cl2(g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures E) 2.4 mol of NOCl, 2.4 mol of NO, and 1.2 mol Cl2
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