Chemistry gas laws

Question

A sample of potassium chlorate placed in a 20.0-L container decomposes to form potassium chloride and oxygen gas.

2KClO₃(s) → 2KCl(s) + 3O₂(g)

If the sample contained 2.0 moles of KClO₃ at a temperature of 214.0 °C, determine the mass of the oxygen gas produced in grams and the pressure exerted by the gas against the container walls.

Answer 1

2 mol KClO3 (3mol O2/2mol KClO3)=3 mol O2

3 mol O2 (32g/mol)=96 g O2

PV=nRT

214+273=487 K = T

P(20L)=3(0.08206)(487)

Solve for P, which is in atm due to R

P=5.9945

P=6.00 atm