The volume of `2.8g` of `CO` at `27^(@)C` and `0.821 atm` pressure is `(R=0.0821` lit. atm `mol^(-1)K^(-1))`

The volume of 2.8g of carbon monoxide at 27^@C and 0.821 atm pressure is (R= 0.0821 "lit-atm" mol^(-1) K^(-1))

The volume of 2.8g of CO at 27°C and 0.821 atm pressure is (R = 0.0821 l atm Km^(-)ol^(-) )

The volume of 2.89 g of carbon monoxide at 27^(@)C and 0.821 atm pressure is

The volume of 2.89 g of carbon monoxide at 27^(@)C and 0.821 atm pressure is

The volume of 2.8 g of carbon monoxide at 27^(@) C and 0.821 atm pressure (R = 0.821 "atm" K^(-1) "mol"^(-1))

What is the molar mass of a gas whose density is 1.5 g L^(-1) at 27^(@)C and 1 atm pressure ? (Use R = 0.08L atm mol^(-1) K^(-1) )

The density of O_2 gas at 127^o C and 4.0 atm pressure is (R = 0.082 L atm K^-1 mol^-1 )

Density of methane , at 250^(@)C and 6 atm pressure, is [R=0.0821 atm ] :