Answer to Question #252029 in General Chemistry for Paul

Question #252029

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?


1
Expert's answer
2021-10-16T02:01:52-0400

m=1.25  gV=750  mL=0.75  LT=22.5+273.15=295.65  KM(CO2)=44.01  g/moln(CO2)=1.2544.01=0.0284  molm=1.25 \;g \\ V=750 \;mL = 0.75 \;L \\ T= 22.5+273.15 = 295.65 \;K \\ M(CO_2) = 44.01 \;g/mol \\ n(CO_2) = \frac{1.25}{44.01} = 0.0284 \;mol

Ideal gas law

pV = nRT

R = 0.08206 L×atm/mol×K

p=nRTVp=0.0284×0.08206×295.650.75=0.918  atmp=\frac{nRT}{V} \\ p= \frac{0.0284 \times 0.08206 \times 295.65}{0.75} = 0.918 \;atm

Answer: 0.918 atm


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