Heat of Reaction
Trending Questions
Q. Consider the reactions
C(s)+2H2(g)⟶CH4(g), ΔH=−x kcal
C(g)+4H(g)⟶CH4(g), ΔH=−x1 kcal
CH4(g)⟶CH3(g)+H(g), ΔH=+y kcal
The average bond energy of C−H bond in methane is
C(s)+2H2(g)⟶CH4(g), ΔH=−x kcal
C(g)+4H(g)⟶CH4(g), ΔH=−x1 kcal
CH4(g)⟶CH3(g)+H(g), ΔH=+y kcal
The average bond energy of C−H bond in methane is
- x4 kcal mol−1
- x1 kcal mol−1
- x14 kcal mol−1
- y kcal mol−1
Q. Heat produced in calories by the combustion of one gram of carbon is called
- Heat of combustion of carbon
- Heat of formation of carbon
- Calorific value of carbon
- Heat of production of carbon
Q.
Consider the following data:
ΔfH0 (N2H4, l) = 50 kJ/mol
ΔfH0 (NH3, g) = −46k J/mol
B.E.(N−H) = 393 kJ/mol and B.E.(H−H) = 436 kJ/mol, also ΔvapH(N2H4, l) = 18 kJ/mol
The N- N bond energy in N2H4 is
226 kJ/mol
154 kJ/mol
190 kJ/mol
45.45 kJ/mol
Q. If the heat of dissolution of an.CuSO4 and CuSO4.5H2O are (-15.89) kcal and 2.80 kcal respectively. Calculate the heat of hydration of CuSO4:
- 18.69 kcal
- -13.09 kcal
- -18.69 kcal
- 13.09 kcal
Q. The heats of combustion of rhombic and monoclinic sulphur are 70960 and 71030 cal/mol respectively. Calculate the heat of conversion of rhombic to monoclinic sulphur
- 70960 cal
- - 70 cal
- 71030 cal
- 70 cal
Q. The enthalpy of solution of BaCl2(s) and BaCl2.2H2O(s) are – 20.6 and 8.8 kJ mol−1 respectively, the enthalpy change for the hydration of BaCl2(s) is:
- – 29.4 kJ
- + 11.8 kJ
- – 11.8 kJ
- 29.4 kJ
Q. Bond dissociation enthalpies of H2(g), Cl2 and HCl(g) are 104, 58 and 103 kcal respectively. The enthalpy of formation of HCl is
- - 44 kcal
- - 88 kcal
- - 22 kcal
- - 11 kcal
Q. The enthalpy change in the reaction, 2CO + O2⟶2CO2 is termed as:
Enthalpy of reaction
Enthalpy of combustion
Enthalpy of formation
Enthalpy of fusion
Q.
Heat of reaction for C6H12O6(s) + 6O2 → 6CO2(g) + 6H2O(v) at constant pressure is −651 K cal at 17∘ C. What is the heat of reaction at constant volume at 17∘ C?
-654.48 Kcal
-655.48 Kcal
-653.48 Kcal
None of these
Q. Given, C(graphites)+O2(g)→CO2(g)
Δr H∘=−393.5 kJ mol−1
H2(g)+12 O2(g)→H2O(l);
ΔrH∘=−285.8 kJ mol−2
CO2(g+2H2O(l)→CH4(g)+2O2(g)
ΔrH∘=+890.3 kJ mol−1
Based on the above thermochemical equations, the value of Δr H∘ at 298K for the reaction, C(graphite)+2H2(g)→CH4(g) will be
Δr H∘=−393.5 kJ mol−1
H2(g)+12 O2(g)→H2O(l);
ΔrH∘=−285.8 kJ mol−2
CO2(g+2H2O(l)→CH4(g)+2O2(g)
ΔrH∘=+890.3 kJ mol−1
Based on the above thermochemical equations, the value of Δr H∘ at 298K for the reaction, C(graphite)+2H2(g)→CH4(g) will be
- +144.0kJmol(−1)
- −74.8kJmol(−1)
- −144.0kJmol(−1)
- +78.8kJmol(−1)