The volume of 2 mole `CO_2` gas at `27^@C` temperature is `0.001 m^3`. Calculate the pressure of this, gas by applying Ideal gas equation Given that, in case of `CO_2, a = 0.364 Nm^4 mol^-1` b = `4.27 xx10^-5 m^3 mol^-1`

Volume of 2 moles of CO_(2) gas at 27^(@)C is 0.001 m^(3) . What will be the pressure of this gas (i) according to van der waals equation and (ii) according to ideal gas equation? [Given a(CO_(2))=0.364" "N*m^(4)*mol^(-2) and b(CO_(2))=4.27xx10^(-5)m^(3)*mol^(-1) ]

Calculate the pressure exerted by 5 moles of CO_2 in one litre vessel at 47^@ C using Vanderwaal's equation. Also report the pressure of gas if it behaves ideally in nature. Given that a=3.592 atm lit^2 mol^(-2) . b = 0.0427 lit mol^(-1)

Calculate the pressure exerted by 5 mole of CO_2 in one litre vessel at 47^@C using van der Waals equation. Also report the pressure of gas if it behaves ideal in nature. Given that a = 3.592 atm L^2mol^(-1),b=0.0427Lmol^(-1) . Also, if the volume occupied by CO_2 molecules is negligible, then calculate the pressure exerted by one mole of CO_2 gas at 273 K.

Volume of a gas at 27^@C is 2 litre keeping pressure constant at what temperature does the volume of the gas become 3 litre?

22g of CO_2 gas at 27^@C is mixed with 16 g of O_2 gas at 37^@C . What will be the temperature of the mixture?

Calculate the temperature of 4.0 moles of a gas occupying 5dm^3 at 3.32 ber. (R = 0.083 bar dm^3K^(-1)mol^(-1)

The van der Waals' constants of a gas are a=0.687dm^2mol^(-2)b=0.0226dm^3mol^(-1)

At 27^@C temperature a gas occupies 2L. In which temperature at constant pressure it will occupy 3L.

The pressure of 3 mol of an ideal gas is 10 atm at 27^(@)C . Calculate work done by the gas when it is expanded isothermally against an external pressure of 1 atm.