![SOLVED:Rearrange the van der Waals equation to solve for P . Why is the pressure exerted by a real gas lower than the pressure for an ideal gas at the same temperature SOLVED:Rearrange the van der Waals equation to solve for P . Why is the pressure exerted by a real gas lower than the pressure for an ideal gas at the same temperature](https://cdn.numerade.com/previews/aa6156c8-326e-4da6-b034-11a301900b0d_large.jpg)
SOLVED:Rearrange the van der Waals equation to solve for P . Why is the pressure exerted by a real gas lower than the pressure for an ideal gas at the same temperature
![For real gases van der Waals equation is written as ( P + an^2/V^2 )(V - nb) = nRT Where 'a' and 'b' are van der Waals constants.Two sets of gases are :( For real gases van der Waals equation is written as ( P + an^2/V^2 )(V - nb) = nRT Where 'a' and 'b' are van der Waals constants.Two sets of gases are :(](https://dwes9vv9u0550.cloudfront.net/images/9485176/bc8cc94c-a20e-4874-b8bf-64a067a6c53f.jpg)
For real gases van der Waals equation is written as ( P + an^2/V^2 )(V - nb) = nRT Where 'a' and 'b' are van der Waals constants.Two sets of gases are :(
For real gas van der Waals equation is written as: ( p + an^2V^2 ) ( V - nb ) = nRT Where a and b are van der Waals constants.Two sets
![The Van der Wall equation for 1 mole of a real gas is ( P + a/V^2 )(V - b) = RT where P is the pressure, V is the volume, T The Van der Wall equation for 1 mole of a real gas is ( P + a/V^2 )(V - b) = RT where P is the pressure, V is the volume, T](https://dwes9vv9u0550.cloudfront.net/images/1218340/ea121fde-df2a-43dc-b290-ef73640ffe12.jpg)