What is the pressure of a 59.6-l gas sample containing 3.01 mol of gas at 44.9°c? (r = 0.0821 l • atm/(k • mol), 1 atm = 760 torr)?

Presuming that the gas behaves like an ideal gas: Volume in cubic meter V= 59.6x 0.001= 0.0596 mÂł n=3.01 mol Temperature in Kelvin T=44.9+273.15=318.05 K R= 8.413 J/ mol K The ideal gas law: PxV= nxRxT Substituting the give information from the question into the ideal gas law: P= 3.01 mol x 8.413 J/mol k x 318.05 K / 0.0596= 133544.392 Pa 1351.3458 Pa / 101325 Pa/ atm = 1.3179806 atm