[" Calculate the pressure exerted by "5" moles of "CO_(2)" in one litre vessel at "47^(@)C" using van der Waal's "],[" equation.Given "a=3.592" atm litre "^(2)" mol "^(2),b=0.0427" litre mol "^(-1)" ."]

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 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))

Calculate the pressure excerted by 5 mol of CO_(2) in 1 L vessel at 47^(@)C using van der Waals equation. Also report the pressure of gas if it behaves ideally in nature. (a=3.592 atm L^(2) mol^(-2), b=0.0427 L mol^(-1))

Pressure exerted by 1 mole of methane, in a 0.25 litre container at 300K using van der Waals' equation (given a= 2.253 atm L^(2) mol^(-2), b= 0.0428L mol^(-)) is

Pressure exerted by 1 mole of methane in a 0.25 litre container at 300K using Vander Waal’s equation : (Given : a = 2.253 "atm" l^(2) "mol"^(-2) and b = 0.0428 l "mol"^(-1) ) is

Pressure exerted by 1 mole of methane in a 0.25 litre container at 300K using Vander Waal’s equation : (Given : a = 2.253 "atm" l^(2) "mol"^(-2) and b = 0.0428 l "mol"^(-1) ) 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.