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 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 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 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.

A gas mixture composed of N_(2) and O_(2) gases has a density of 1.17g*L^(-1) at 27^(@)C and 1 atm pressure. Calculate the mass percents of N_(2) and O_(2) in the mixture. Assume that the gas mixture behaves like an ideal gas.

One mole of carbon-dioxide was found to occupy a volume of 1.32 litre at 48^(@) C and at a pressure of 16.4 atm. Calculate the pressure of the gas that would have been expected to behave ideally and non-ideally.

The pressure exerted by 12 g of an ideal gas at temperature t^@C in a vessel of volume V litre is one atm.when the temperature is increased by 10 degree at the same volume.the pressure increases by 10% calculate the temperature t and volume v.(molecular weight of the gas =120).

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

Calculate the pressure required to compress a gas adiabatically at atmospheric pressure to one third of its volume. Given gamma = 1.47 .

Calculate the total pressure in a mixture of 8 g oxygen and 4g of hydrogen confined in a vessel of 1 dm^3 at 27^@C. (R=0.083 bar dm^3k^(-1) mol^(-1))

Calculate the work done when 1 mol of water vaporises at 100^(@)C and 1 atm pressure. Assume water vapour behaves like an ideal gas.