The heats of neutralisation of four acids A, B, C and D are -13.7, -9.4, -11.2 and -12.4 kcal respectively when they are neutralised by a common base. The acidic character obeys the order :
1. A>B>C>D
2. A>D>C>B
3. D>C>B>A
4. D>B>C>A
The for CO2(g), CO(g) and H2O(g) are -393.5, -110.5 and -241.8 kJ mol-1 respectively. The standard enthalpy change (in kJ) for the reaction,
is :
1. 524.21
2. 41.2
3. -262.5
4. -41.2
The dissociation energy of CH4 and C2H6 are respectively 360 and 620 Kcal/mole. The bond energy of C-C is-
1. 260 Kcal/mole
2. 180 Kcal/mole
3. 130 Kcal/mole
4. 80 Kcal/mole
All the natural process in this universe produce
1. A decrease in entropy of the universe
2. An increase in entropy of the universe
3. No change in entropy
4. Sometimes increase or sometimes decrease in entropy
For the reaction, , at 298K is 164 kJ mol-1. The of the reaction is-
1. \(166.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
2. \(141.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
3. \(104.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
4. \(-169 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
For \(A \rightarrow B\), \(\Delta H = 4\ kcal\ mol^{-1}\), \(\Delta S = 10\ cal\ mol^{-1}\ K^{-1}\), the reaction is spontaneous when the temperature is:
1. 400 K
2. 300 K
3. 500 K
4. None of the above
44.0 kJ of heat is required to evaporate one mole of water at 298 K. If of is -286 kJ mol-1, of is
1. -330 kJ mol-1
2. +242 kJ mol-1
3. -242 kJ mol-1
4. -198 kJ mol-1
The correct calculate value for for:
From following arbitrary values :
1. 1950 KJ mol-1
2. 1150 KJ mol-1
3. 2300 KJ mol-1
4. None of the above.
The molar heat capacity, of an ideal gas whose energy is that of translational motion only is
1.
2.
3.
4.