A(g) + B(g) --> C(g)

for which K = 1.3X10^2. Assume that 0.406 mol C(g) is placed inthe cylinder represented below. The temperature is 300.0 K, and htebarometric pressure on the piston (which is assumed to be masslessand frictionless) is constant at 1.00 atm. the original volume(before te 0.406 mol C(g) begins to decompose) is 10.0 L. What isthe volume on the cylinder at equilibrium?

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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)

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redrabbit267

Needing help with 36,46, 68, and 72.

A gaseous material l, XY(g) , dissociates to some extent to produce X(g) and Y(g).

XY(g) â X(g) + Y(g) K_c = 5.53 x 10^-3

A 2.00 gram sample 0f XY(M_w = 165g/mol) is placed in a container with a movable piston at 25^oC. The atmospheric pressure is 0.967 atm. Assume the piston is massless and frictionless. As XY(g) dissociates the piston moves keeping the pressure constant. Assuming ideal behavior, calculate the following:

a- The volume of the container at equilibrium

b- The percent dissociation of XY

c- The density of the gas mixture at equilibrium