Calculate the pressure exerted by one mole of `CO_2` gas at 273 K, if the Vander Waals constant a = 3.592` dm^6 atm mol^(−2)` . Assume that the volume occupied by `CO_2` molecules is negligible.

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.

Calculate the pressure exerted by 5 mol of CO_2 in one litre vessels at 47^@C If it behaves ideally in nature.

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 partial pressure of SO_2 in a mixture with 60% CO_2 and total pressure being 4 atm.

Calculate the volume of 3.6g of water vapour at 273K temperature and 1 atm pressure.

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

Is the volume of 1 gram-mole of CO_(2) greater than, equal to or less than 22.4 L at 300 K and 1 atm?

The density of O_(2) gas at 1 atm pressure and 273 K is 1.429 g*dm^(-3) . Calculate the root mean square velocity of O_(2) molecule at 273 K?

The inversion temperature Ti(K) of hydrogen is (Given van der Waal’s constant a and b are 0.244 atm L^2 mol^(-2) and 0.027 L mol^(-1) respectively.)