A 4.40 g piece of solid CO2 (dry ice) is allowed to vaporize in a balloon. The final volume of the balloon is 1.00 L at 300. K. What is the pressure of the gas?
4.40 g = 0.1 moles CO2
So now we have to find P such that
1.00P/300 = 0.1*22.4*1/273
P = 2.46 atm
Correct! Just one small correction, the final volume of the balloon should be 22.4 L (not 1 L) as that is the molar volume of gases at standard temperature and pressure (STP). So the calculation would be:
PV = nRT
P(22.4 L) = (0.1 mol)(0.0821 L·atm/mol·K)(300 K)
P = (0.1 mol)(0.0821 L·atm/mol·K)(300 K)/(22.4 L)
P = 2.46 atm