From the graph of `(d)/(P)` vs P at a constant temperature of 300K. Calculate molar mass of the gas.
[Give R=0.0821 atm lit/mole-k]

From the graph of (d)/(P) us P at a constant temperature of 300 K. calculate molar mass of the gas.

Density of ideal gas at 2.46 atm and 300 K is 0.8 g//L Hence g-molar mass of gas is : [R = 0.082 "L-atm/mol-K"]

The density of a gas is found to be 3.43 g/litre at 300K and 1.00 atm pressure. Calculate the molar mass of the gas.

A container consists of 1 mole of liquid water and 1 mole of N_(2)(g) , at a temperature of 300K. If aqueous tension of water at 300K is 38mm of Hg and the contaienr is fitted with a piston operating at 0.1321 atm then calculate volume occupied by N_(2) gas: (R=0.0821atm L/molk)

At a constant pressure P, the plot of volume (V) as a function of temperature (T) for 2 moles of an ideal gas gives a straight line with a slope 0.328 L K^(-1) . The value of P (in atm) is closest to [Gas constant, R = 0.0821 L atm mol^(-1)" "K^(-1) ]

Calculate the molar concentration of urea solution if it exerts an osmotic pressure of 2.45 atmosphere at 300K . (R=0.0821L atm mol^-1 K^-1 )