A gas having molecular mass `84.5 g mol^(-1)` enclosed in a flask at `27^(@)C` has a pressure of `1.5 "bar"`. Calculate the density of the gas under the same conditions.

A gas having a molecular mass of 84.5 g mol^(-1) enclosed in a flask at 27^(@)C has a pressure of 1.5 atm . Calculate the density of the gas.

A gas of molar mass 84.5g/mol is enclosed in a flask at 27^(@)C has a pressure of 2 atm. Calculate the density of the gas. [R=0.082 *atm*K^(-1)*mol^(-1) ]

A gas of molar mass 84.5 g//mol is enclosed in a flask at 27^@C has a pressure of 2 atm. Calculate the density of the gas. [R = 0.082 L atm K^(-1) mol^(-1)]

The density of a gas at 27^(@)C and 1 bar pressure is "2.56 g L"^(-1) . Calculate the molar mass.

The density of a gas at 27^@C and 1 bar pressure is 2.56 gL^-1 .Calculate the molar mass.

A gas of molecular mass 71 g mol^(-1) is enclosed in a vessel at a temperature of 30^@C . If the pressure exerted by the gas is 1065 mm of Hg, calculate the density of the gas.

2.5gms. of a gas is present in 750ml. flask at 32^@C and 770mm, of Hg pressure. Calculate the molecular mass of the gas.

The vapour of phosphine gas at 27^(@)C and 3 bar pressure has density:

The density of a gas is found to be 1.56 g dm^(-3) at 0.98 bar pressure and 65^(@)C . Calculate the molar mass of the gas.

The density of a gas is found to be 1.56 g dm^(-3) at 0.98 bar pressure and 65^(@)C . Calculate the molar mass of the gas.