<p>Hello I'm an ap chem student, and I'm having great difficulty with one particular marathon problem in chapter 13 #83... I was hoping that someone could give me some pointers. Thanks!</p>
<p>Consider the reaction
A(g) + B(g) <--> C(g) for which K= 1.30 x 10^2. Assume that 0.406 mol C(g) is placed in the cylinder represented below. The temperature is 300.0K, and the barometric pressure on the piston (which is assumed to be massless and frictionless) is constant at 1.00 atm. The original volume (before the 0.406 mol C(g) begins to decompose) is 10.00 L. What is the volume in the cylinder at equilibrium?</p>
<p>There's a picture of a cylinder with a lid with 1.00 atm pressure pushing downwards on it. Also it labels the original volume = 10.00 L, T= 300.0K, and 0.406 mole of pure C(g) (initially).</p>
<p>Thanks again!</p>