Vanderwaal real gas constants
1 . NH 3 2 . N 2 3 . CH 2 Cl 2 4 . Cl 2 5 . CCl 4
Predict which of the above gases have:
(i) the smallest van der Waals "a" constant
(ii) the largest "b" constant.
Concatenate the answer, for an example if gas 1 . NH 3 fits part (i) and gas 4 . Cl 2 fits the part (ii), then enter the answer as 14. For a and b refer van der waal
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1 solution
Thats a nice question. I had a hard time figuring out which had greater Van der Waals constant
C
H
X
2
Cl
X
2
or
C
Cl
X
4
. (+1) for explanation. Can you tidy up this question a bit by adding five to six
_
signs. For example, if you input
_____
a new section would be created between the question and onstruction to submit answer part.
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I have posted as a report myself as I dont know how to leave spaces
You can post report too
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Nono, its not really report. Moderators would edit it as soon as they see it.
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@Ashish Menon – Ok I have posted it as a report. You can see.
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@Prince Loomba
–
Instead of writing
submit your answer as a code
it might be better to write
concatenate your answer
.
(i) N2 The value of the Van der Waals constant, a, of a given gaseous substance depends on the strength of attractions between its component molecules. Molecules experiencing the weakest attractive forces will have the smallest a constant while those with the strongest attractive forces will have the largest a values.
Of the molecules NH3, N2, CH2Cl2, Cl2, CCl4, the two elements nitrogen and chlorine alone have non-polar bonds between their component atoms. This results is weaker attractions between molecules, so N2 and Cl2 will have the smallest a values. The remaining molecules all have polar bonds between their component atoms and in the case of NH3, hydrogen bonds between molecules. These are factors that lead to increased a constants. As the N2 molecule is smaller than the Cl2 molecule and therefore has less electrons present, the attractive forces between N2molecules will be weaker than those between Cl2 molecules and N2 will have the smallest a constant.
(ii) CCl4 The value of the Van der Waals b constant is merely the actual volume of a mole of the molecules and this can be deduced by comparing the volumes of the molecules in the list. Small molecular volume results in small b values and a large molecular volume corresponds to a large b constant. From the compound in the list, CCl4 is the largest and so it will have the greatest b constant.