Ask a New Question

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.

Ask a New Question or answer this question.

Similar Questions

when 2g of a gas A is introduced into an evacuated flask kept at25 centigrade, the pressure is found to be 1 atmosphere.if 3g of
1. 1 answer
At 668K 1 mol each of CO and Cl2 are introduced into an evacuated 1.75 L flask. At equilibrium, the total pressure of the
1. 1 answer
A sample of gaseous PCl5 was introduced into an evacuated flask so that the pressure of pure PCl5 would be 0.54 atm at 425 K.
1. 1 answer
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
1. 1 answer

more similar questions