If volume occupied by `CO_(2)` molecules is negligible, then calculate pressure `((P)/(5.277))` exerted by one mole of `CO_(2)` gas at `300 K`. `(a=3.592 atm L^(2)mol^(-2))`

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 (a=3.592 atm "litre"^(-2)mol^(-2) )

If volume occupied by CO_2 molecules is negligible, then the pressure exerted by one mole of CO_2 gas in terms of temperature (T), assuming V to be single valued, is

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 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))

Which of the following is the correct set of volume calculated by ideal gas equation and van der Waals equation respectively for 1 mole CO_(2) gas at 300 K and 10 atm pressure. (R= 0.0821 L atm K^(-1)mol^(-1))

The pressure exerted by 1 mol of CO_(2) at 273 K is 34.98 atm . Assuming that volume occupied by CO_(2) molecules is negligible, the value of van der Waals constant for attraction of CO_(2) gas is

The pressure exerted by 1 mol of CO_(2) at 273 K is 34.98 atm . Assuming that volume occupied by CO_(2) molecules is negligible, the value of van der Waals constant for attraction of CO_(2) gas is

Calculate the volume occupied at S.T.P. by 2 moles of CO_(2)