1
AIEEE 2006
MCQ (Single Correct Answer)
+4
-1
The enthalpy changes for the following processes are listed below :

Cl2(g) = 2Cl(g), 242.3 kJ mol–1
I2(g) = 2I(g), 151.0 kJ mol–1
ICl(g) = I(g) + Cl(g), 211.3 kJ mol–1
I2(s) = I2(g), 62.76 kJ mol–1

Given that the standard states for iodine and chlorine are I2(s) and Cl2(g), the standard enthalpy of formation for ICl(g) is :
A
–14.6 kJ mol–1
B
–16.8 kJ mol–1
C
+16.8 kJ mol–1
D
+244.8 kJ mol–1
2
AIEEE 2005
MCQ (Single Correct Answer)
+4
-1
Consider an endothermic reaction, X $$\to$$ Y with the activation energies Eb and Ef for the backward and forward reactions, respectively. In general :
A
Eb < Ef
B
Eb > Ef
C
Eb = Ef
D
There is no definite relation between Eb and Ef
3
AIEEE 2005
MCQ (Single Correct Answer)
+4
-1
Consider the reaction: N2 + 3H2 $$\to$$ 2NH3 carried out at constant temperature and pressure. If $$\Delta H$$ and $$\Delta U$$ are the enthalpy and internal energy changes for the reaction, which of the following expressions is true?
A
$$\Delta H$$ > $$\Delta U$$
B
$$\Delta H$$ < $$\Delta U$$
C
$$\Delta H$$ = $$\Delta U$$
D
$$\Delta H$$ = 0
4
AIEEE 2005
MCQ (Single Correct Answer)
+4
-1
If the bond dissociation energies of XY, X2 and Y2 (all diatomic molecules) are in the ratio of 1:1:0.5 and $$\Delta H_f$$ for the formation of XY is -200 kJ mole-1. The bond dissociation energy of X2 will be :
A
100 kJ mol-1
B
200 kJ mol-1
C
300 kJ mol-1
D
800 kJ mol-1
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