Calculate the volume occupied by 8.8g of `CO_2` at `31.1^@C` and 1 bar pressure.R=0.83bar `Dm^3.k^1 mol^(-1)`

Calculate the volume occupied by 8.8 g of CO_(2) at 31.1^(@)C & 1 bar pressure. R=0.083 bar *L*K^(-1)mol^(-1) .

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

At 25^(@)C and at a certain pressure, 3.7 g of a gas occupies the same volume as the volume occupied by 0.184 of H_(2) gas at 17^(@)C and the same pressure. Calculate molar mass of the gas.

Calculate the temperature of 4.0 moles of a gas occupying 5dm^3 at 3.32 ber. (R = 0.083 bar dm^3K^(-1)mol^(-1)

Calculate the temperature of 4.0 mol of gas occupying 5 dm^(3) at 3.32 bar. (R=0.083 bar *dm^(3)*K^(-1)*mol^(-1) )

Bar is a unit of pressure. 1 bar = ?

Calculate the value of enthalpy of combustion of cyclopropane at 25^(@)C and 1 atm pressure. Given: Standard enthalpy of formation of CO_(2)(g),H_(2)O(l) & propene (g) at 25^(@)C are -393.5kJ*mol^(_1),-285.8kJ*mol^(-1)& 20.4kJ*mol^(-1) respectively. also standard enthalpy change for isomerisation reaction: Cyclopropane (g) hArr Propene (g) is -33.0kJ*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.

What will be the volume of one mole of oxygen at 27^@C and at a pressure twice the standard atmosphere R=8.31 times 10^7 erg.mol^-1K^-1 .

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)