The correction terms in the Van der Waals equation for a gas are designed to correct
A. the pressure term (P +a/V2) for the attractive forces between particles.
B. the volume term (V-b) for the finite volume of the particles.
C. For the volume term (b) not the pressure term (a).
D. For both the pressure term (a) and the volume term (b).
(Broken Link Removed)
I tried the link Bob Pursley gave you and received an error notice. Here is another link that may help.http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch4/deviation5.html
To determine the correct answer to the question, let's consider the components of the Van der Waals equation.
The Van der Waals equation is an equation of state that improves upon the ideal gas law by accounting for the intermolecular forces and molecular volume of real gases.
The equation is represented as:
(P + a(n/V)^2)(V - nb) = nRT
Here, P represents the pressure, V represents the volume, n represents the number of moles of gas, R is the ideal gas constant, and T is the temperature.
The Van der Waals equation includes two correction terms: a/V^2 and nb.
The term a/V^2 adjusts for the attractive forces between particles in a gas. This term accounts for the fact that gas molecules attract each other, causing the pressure in the system to be slightly lower than what would be predicted by the ideal gas law.
The term nb corrects for the finite volume occupied by gas molecules. Since gas molecules have a non-zero size, the actual volume available for molecular movement is less than the total volume of the container. This correction term accounts for this reduced available volume.
Now, let's consider the options:
A. The pressure term (P + a/V^2) is indeed corrected for the attractive forces between particles. This term compensates for the attractive forces by adding the correction factor a/V^2 to the pressure term.
B. The volume term (V - nb) is corrected for the finite volume of the particles. This correction factor accounts for the molecular volume by subtracting nb from the volume term.
C. This option states that the correction is only applied to the volume term (b), and not the pressure term (a). However, this is incorrect as both terms are corrected in the Van der Waals equation.
D. This option correctly states that both the pressure term (a) and the volume term (b) are corrected.
From the explanation above, we can determine that the correct answer is D. The correction terms in the Van der Waals equation are designed to correct both the pressure term (P + a/V^2) and the volume term (V - nb) for the attractive forces between particles and the finite volume occupied by gas molecules, respectively.