A sample of an unknown compound is vaporized at 150.Â°C . The gas produced has a volume of 960.mL at a pressure of 1.00atm , and it weighs 0.941g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

The molar mass of a chemical compound is defined as the mass of a sample of that compound divided by the number of moles in that sample. Its unit of measurement is grams per mole (g/mol) although in the International System of Measurements it should be kilograms per mole (kg/mol).

This is a property closely related to the relative molar mass of a compound and to the standard atomic masses of the constituent elements.

Determination of the molar mass of the unknown gas

To determine the molar mass of the gas, the ideal gas equation was used: PV = nrt, in which

P = Pressure

V = Volume

n = number of moles

R = Gas constant

t = temperature

But previously the moles of the gas are calculated

Calculate the moles of the unknown compound

Data

t = 150°C = 423.15K

V = 960ml = 0.96L

P = 1.00 atm

R = 0.082 L Atm / mol °K .

n = ?

PV = nrt

n = PV/rt

n=1. 0.96 / 0.082. 423.15

n = 0.96 / 34.7

n = 0.027 mole

Calculation of the molar mass of the unknown compound

M = m/n

M = 0.94 g/ 0.027 mol

M = 34.81 g/mol

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