Pressure exerted by `1` mole of methane, in a `0.25` litre container at `300K` using van der Waals' equation (given `a= 2.253 atm L^(2) mol^(-2), b= 0.0428L mol^(-))` is

Pressure exerted by 1 mole of methane in a 0.25 litre container at 300K using Vander Waal’s equation : (Given : a = 2.253 "atm" l^(2) "mol"^(-2) and b = 0.0428 l "mol"^(-1) ) is

Pressure exerted by 1 mole of methane in a 0.25 litre container at 300K using Vander Waal’s equation : (Given : a = 2.253 "atm" l^(2) "mol"^(-2) and b = 0.0428 l "mol"^(-1) ) is

Calculate the pressure excerted by 5 mol of CO_(2) in 1 L vessel at 47^(@)C using van der Waals equation. (a=3.592 atm L^(2) mol^(-2), b=0.0427 L mol^(-1))

Calculate the pressure exerted by 16 g of methane in a 250 mL container at 300 K using van der Waal's equation. What pressure will be predicted by ideal gas equation ? a = 2.253 atm L^(2) mol^(-2), b = 0.0428 L mol^(-1) R = 0.0821 L atm K^(-1) mol^(-1)

88 g of CO_2 are confined to a 6 L flask at 37^@C . Calculate its pressure using van der Waals' equation. Given, a = 4.17 " atm " L^2 mol^(-2), b = 0.038 L mol^(-1) .

Calculate the pressure exerted by one mole of methane in a 450 mL container at 25^@C using van der Waals' equation. What pressure will be predicted by ideal gas equation ? (Given : a = 2.253 " atm " L^2 mol^(-2), b = 0.0428 L mol^(-2), R =0.0821 L " atm " K^(-1) mol^(_1))

Two moles of ammonia were found to occupy a volume of 5 L at 27^(@)C . Calculate the pressure using van der Waals equation (a="4.17 bar L"^(2)"mol"^(-2), b="0.0371 L mol"^(-1)).

Calculate the pressure exerted by 0.350 moles of carbon dioxide in 0.360 L container at 100^@C . What pressure will be predicted by ideal gas equation? (a = 3.59 " atm " L^2 mol^(-2), b = 0.0427 L mol^(-1) )

A vessel of 25 litre capacity contains 10 moles of steam under pressure of 50.3 atm. Calculate the temperature of steam using van der Waals equation (if for water a=5.46 bar L^2 mol^(-2) and b=0.031 L mol^(-1) )