Home
Class 11
CHEMISTRY
Calculate the pressure exerted by 10.2g ...

Calculate the pressure exerted by 10.2g of `NH_(3) 3 dm^(3)` vessel at `25^(@)C` (a) using ideal gas equation (b) using van der Waals equation . The van der Waals constants are : `a=4.17 dm^(6)" atm"mol^(-2),b=0.0371 dm^(3)mol^(-1)`

Promotional Banner

Similar Questions

Explore conceptually related problems

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

Calculate the pressure exerted by 22g of CO_(2) in 0.5 dm^(3) at 300 K using ( a ) the ideal gas law and ( b ) the van der Waals equation. Given a=300.0 kPa dm^(6) mol^(-2) and b=40.0 cm^(3) mol^(-1) .

Calculate the pressure exerted by 22g of CO_(2) in 0.5 dm^(3) at 300 K using ( a ) the ideal gas law and ( b ) the van der Waals equation. Given a=300.0 kPa dm^(6) mol^(-2) and b=40.0 cm^(3) mol^(-1) .

Calculate the critical constants of a gas whose van der Waals constants are : a=0.751" L"^(2)" atm "mol^(-2) and b=0.0226" L mol"^(-1) .

The ratio (a/b) (the terms used in van der Waals’equation) has the unit :

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))

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))