Calculate the pressure exerted by `22g` of `CO_(2)` in `0.5 dm^(3)` at `300 K` using (`a`) the ideal gas law and (`b`) the van der Waals equation. Given `a=300.0 kPa dm^(6) mol^(-2)` and `b=40.0 cm^(3) mol^(-1)`.

Calculate the pressure exerted by 10.2g of NH_(3) 3 dm^(3) vessel at 25^(@)C (a) using ideal gas equation (b) using van der Waals equation . The van der Waals constants are : a=4.17 dm^(6)" atm"mol^(-2),b=0.0371 dm^(3)mol^(-1)

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

One mole of CO_(2) occpuies 1.5 L at 25^(@)C . Calculate the pressure exerted by the gas using (i) ideal gas equation van der Waals gas equation with a=3.6 L^(2)" bar mol"^(-2) and b="0.04 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.

Assuming CO_(2) to be van der Waals gas, calculate its Boyle temperature. Given a=3.59" L"^(2)" atm " mol^(-2) and b=0.0427" L "mol^(-1) .