what volume would 120.0g of nitrogen gas occupy at 59.50 c and 0.566 atm
59.50oC = 59.50 + 273.15 = 332.65 K
n(N2)=120.0 g28.01 g/mol=4.284 moln(N_2)=\frac{120.0\ g}{28.01\ g/mol}=4.284\ moln(N2)=28.01 g/mol120.0 g=4.284 mol
R=0.08206L⋅atmmol⋅KR=0.08206\frac{L\cdot{atm}}{mol\cdot{K}}R=0.08206mol⋅KL⋅atm
According to the ideal gas law,
PV=nRTPV=nRTPV=nRT ;
V=nRTP=4.284 mol×0.08206L⋅atmmol⋅K×332.65 K0.566 atm=207 LV=\frac{nRT}{P}=\frac{4.284\ mol\times0.08206\frac{L\cdot{atm}}{mol\cdot{K}}\times332.65\ K}{0.566\ atm}=207\ LV=PnRT=0.566 atm4.284 mol×0.08206mol⋅KL⋅atm×332.65 K=207 L
Answer: 207 L
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