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# Calculate each of the following quantities for an ideal gas.?

(a) the volume of the gas, in liters, if 1.89 mol has a pressure of 0.976 atm at a temperature of -6°C

(b) the absolute temperature of the gas at which 3.33 10-3 mol occupies 248 mL at 730. torr

(c) the pressure, in atmospheres, if 0.0485 mol occupies 421 mL at 107°C

(d) the quantity of gas, in moles, if 66.4 L at 50.°C has a pressure of 11.39 kPa

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- Roger the MoleLv 72 years agoFavorite Answer
(a)

V = nRT / P = (1.89 mol) x (0.08205746 L atm/K mol) x (−6 + 273) K / (0.976 atm) = 42.4 L

(b)

T = PV / nR = (730. torr) x (0.248 L) / ((3.33 x 10^-3 mol) x (62.36367 L torr/K mol)) = 872 K

(c)

P = nRT / V = (0.0485 mol) x (0.08205746 L atm/K mol) x (107 + 273) K / (0.421 L) = 3.59 atm

(d)

n = PV / RT = (11.39 kPa) x (66.4 L) / ((8.3144621 L kPa/K mol) x (50. + 273) K) = 0.282 mol

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