A 1.25-g sample of CO2 is contained in a 750.-mL flask at 22.5 °C. What is the pressure
of the gas?
"m=1.25 \\;g \\\\\n\nV=750 \\;mL = 0.75 \\;L \\\\\n\nT= 22.5+273.15 = 295.65 \\;K \\\\\n\nM(CO_2) = 44.01 \\;g\/mol \\\\\n\nn(CO_2) = \\frac{1.25}{44.01} = 0.0284 \\;mol"
Ideal gas law
pV = nRT
R = 0.08206 L×atm/mol×K
"p=\\frac{nRT}{V} \\\\\n\np= \\frac{0.0284 \\times 0.08206 \\times 295.65}{0.75} = 0.918 \\;atm"
Answer: 0.918 atm
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