Question

Consider the reaction

A (g) + B (g) C (g)

for which K = 1.30 x 10 squared. Assume that 0.406 mol C (g) isplaced in the cylinder represented below. The temperature is 300.0K, and the barometric pressure on the piston (which is assumed tobe massless and frictionless) is constant at 1.00 atm. The originalvolume (before the 0.406 mol C (g) begins to decompose) is 10.00 L.What is the volume in the cylinder at equilibrium?

P=1.00 atm

Orignal Volume = 10.00 L

T = 300.0 K

0.406 mole of pure C (g) (initially)

Thanks in advance! Lifesaver Awarded!