Calculate the pressure exerted by `8.5 g` of ammonia `(NH_(3))` contained in a `0.5 L` vessel at `300 K`. For ammonia, `a=4.0 atm L^(2)mol^(-2)`, `b=0.036 L mol^(-1)`.

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))

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

Using the van der Waals equation, calculate the pressure of 10.0mol NH_(3) gas in a 10.0 L vessel at 27^(@)C . {:((P+n^(2)(a)/(V^(2)))(V-nb)=nRT,,a=4.2L^(2).atm//mol^(2),,b=0.037L//mol):}

Using the van der Waals equation, calculate the pressure of 10.0mol NH_(3) gas in a 10.0 L vessel at 27^(@)C . {:((P+n^(2)(a)/(V^(2)))(V-nb)=nRT,,a=4.2L^(2).atm//mol^(2),,b=0.037L//mol):}

2 moles of ammonia occupied a volume of 5 lit at 27^@C . Calculate the pressure if a=4.17atmL^2 mol^(-2), b= 0.0371 L mol^(-1)

Calculate the pressure of 154 g carbon dioxide in a vessel of 2.0 L capacity at 30^(@)C , a = 648 L bar atm K^(-1) mol^(-1), b = 0.0427 L mol^(-1)

Calculate the pressure of 154 g carbon dioxide in a vessel of 2.0 L capacity at 30^(@)C , a = 648 L bar atm K^(-1) mol^(-1), b = 0.0427 L mol^(-1)

Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at 37^(@)C . Given that the van der Waal’s constants are a = 3.59 L^(2) " atm "mol^(-2) and b = 0.0427 L mol^(-1) . Compare the value with the calculated value if the gas were considered as ideal.

Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at 37^(@)C . Given that the van der Waal’s constants are a = 3.59 L^(2) " atm "mol^(-2) and b = 0.0427 L mol^(-1) . Compare the value with the calculated value if the gas were considered as ideal.