What volume would 11.2 g of a gaseous compound occupy at STP if its molecular weight is 44.0 g/mole and it behaves as an ideal gas?

Question

Quizplus · Accepted Answer

The correct answer is A.The volume of a gas at STP can be calculated using the ideal gas law: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. At STP, the pressure is 1 atm, the temperature is 273 K, and the number of moles can be calculated from the mass and molecular weight of the gas.In this case, the mass of the gas is 11.2 g, the molecular weight is 44.0 g/mole, and the number of moles is 11.2 g / 44.0 g/mole = 0.2545 moles.Substituting these values into the ideal gas law, we get:V = nRT/P = (0.2545 moles)(0.0821 Latm/(molK))(273 K)/(1 atm) = 5.71 litersTherefore, the volume of 11.2 g of a gaseous compound with a molecular weight of 44.0 g/mole at STP is 5.71 liters.

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