This chapter is currently out of syllabus
1
JEE Main 2014 (Offline)
+4
-1
Out of Syllabus
If Z is a compressibility factor, van der Waals equation at low pressure can be written as:
A
Z = 1 + $$RT \over Pb$$
B
Z = 1 - $$a \over VRT$$
C
Z = 1 - $$Pb \over RT$$
D
Z = 1 + $$Pb \over RT$$
2
JEE Main 2013 (Offline)
+4
-1
Out of Syllabus
For gaseous state, if most probable speed is denoted by C*, average speed by $$\mathop C\limits^{\_\_}$$ and mean square speed by C, then for a large number of molecules the ratios of these speeds are:
A
C*: $$\mathop C\limits^{\_\_}$$ : C = 1.128 : 1.225 : 1
B
C*: $$\mathop C\limits^{\_\_}$$ : C = 1.225 : 1.128 : 1
C
C*: $$\mathop C\limits^{\_\_}$$ : C = 1 : 1.225 : 1.128
D
C*: $$\mathop C\limits^{\_\_}$$ : C = 1 : 1.128 : 1.225
3
AIEEE 2012
+4
-1
Out of Syllabus
The compressibility factor for a real gas at high pressure is :
A
1 + RT/pb
B
1
C
1 + pb/RT
D
1–pb/RT
4
AIEEE 2011
+4
-1
Out of Syllabus
'a’ and `b’ are van der Waals’ constants for gases. Chlorine is more easily liquefied than ethane because
A
a and b for Cl2 < a and b for C2H6
B
a and b for Cl2 > a and b for C2H6
C
a for Cl2 > a for C2H6 and b Cl2 < b for C2H6
D
a for Cl2 < a for C2H6 and b Cl2 > b for C2H6
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