pV = nRT =>
T = (pV)/(nR)
= (1.76 atm)(0.258 L)/[(0.38 mol)(0.08206 L*atm/molK)]
= about 15K but use a calculator.
Then add on 273.15 to go from Kelvin to Celsius.
T = PV / nR = (1.76 atm) x (0.258 L) / (0.38 mol x (0.082057366 L atm/K mol)) =
14.56 K = −259°C
[Although it is doubtful that the Ideal Gas Equation is still valid at such a low temperature, especially if the gas is anything besides helium.]
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Verified answer
pV = nRT =>
T = (pV)/(nR)
= (1.76 atm)(0.258 L)/[(0.38 mol)(0.08206 L*atm/molK)]
= about 15K but use a calculator.
Then add on 273.15 to go from Kelvin to Celsius.
T = PV / nR = (1.76 atm) x (0.258 L) / (0.38 mol x (0.082057366 L atm/K mol)) =
14.56 K = −259°C
[Although it is doubtful that the Ideal Gas Equation is still valid at such a low temperature, especially if the gas is anything besides helium.]