A van der Waals gas has a = 1.39 L^2 atm mol^-2 and b = 0.0391 L mol^-1. Two moles are placed in a 1.00 L vessel at 300

Question

A van der Waals gas has a = 1.39 L^2 atm mol^-2 and b = 0.0391 L mol^-1. Two moles are placed in a 1.00 L vessel at 300 K (R = 0.0821 L atm K^-1 mol^-1). Which statements are correct?

Accepted Answer

The free volume is 0.9218 L

Accepted Answer

The pressure correction term is 5.56 atm

Accepted Answer

The van der Waals pressure is about 47.9 atm

Accepted Answer

The gas exerts a lower pressure than an ideal gas would

A van der Waals gas has $a = 1.39 L^{2} atm mo l^{- 2}$ and $b = 0.0391 L mo l^{- 1}$ . Two moles are placed in a $1.00 L$ vessel at $300 K$ ( $R = 0.0821 L atm K^{- 1} mo l^{- 1}$ ). Which statements are correct?

Answer: A, B, C, D

More questions on van der Waals equation and its constants

A van der Waals gas has a=1.39 L2atmmol−2 and b=0.0391 Lmol−1. Two moles are placed in a 1.00 L vessel at 300 K (R=0.0821 LatmK−1mol−1). Which statements are correct?

Answer: A, B, C, D

More questions on van der Waals equation and its constants

A van der Waals gas has $a = 1.39 L^{2} atm mo l^{- 2}$ and $b = 0.0391 L mo l^{- 1}$ . Two moles are placed in a $1.00 L$ vessel at $300 K$ ( $R = 0.0821 L atm K^{- 1} mo l^{- 1}$ ). Which statements are correct?