If at 298 K the bond energies of C–H, C–C, C=C and H–H bonds are respectively 414, 347, 615 and 435 kJ mol-1, the value of enthalpy change for the reaction ;
H2C = CH2(g) + H2(g) → H3C–CH3(g) at 298 K will be – [AIEEE-2003]
ΔHReaction = ∑BE Reactant - ∑BE Product
= 4 x 414 + 615 + 435 – (6 x 414 + 347)
= 2706 – 2831
= –125 kJ
The enthalpy change for a reaction does not depend upon -
Hess's Law of Constant Heat Summation states that regardless of the multiple stages or intermediate steps of a reaction, the total enthalpy change for the reaction is the sum of all changes.
The enthalpy of a chemical process is independent of the path taken from the initial to the final state.
The enthalpies of combustion of carbon and carbon monoxide are -393.5 and -283 kJ mol-1 respectively. The enthalpy of formation of carbon monoxide per mole -
C + O2 → CO2
∆Hc = -393.5 kJ/mol -i
CO + ½ O2 → CO2
∆Hc = -283 kJ/mol -ii
C + 1/2 O2 → CO
∆Hf = -110.5 kJ/mol
If the bond dissociation energies of XY, X2 and Y2 (all diatomic molecules) are in the ratio of 1 : 1 : 0.5 and ΔfH for the formation of XY is -200 kJ mol-1. The bond dissociation energy of X2 will be
The standard enthalpy of formation (ΔfHº) at 298 K for methane, CH4(g), is -74.8 kJ mol-1. The additional information required to determine the average energy for C - H bond formation would be -
The correct answer is option D
Carbon is found in the solid-state. The state of the substance affects the enthalpy change.
Hence, the correct option is A
Oxidising power of chlorine in aqueous solution can be determined by the parameters indicated below :
The energy involved in the conversion of Cl2(g) to Cl-(aq)
(using the data, Δdiss
kJ mol-1) will be - [AIEEE 2008]
Oxidising power of chlorine in aqueous solution can be estimated by calculating the overall enthalpy change of reaction.
The reaction takes place with following steps:
1/2Cl2 —> Cl ΔH1
Cl —> Cl− ΔH2
Cl− —> Cl− (aq) ΔH3
ΔH will be the sum of the energy involved in these steps.
Hence, ΔH = ΔH1 +ΔH2 +ΔH3
ΔH1 = 240/2 = 120kJ/mol, ΔH2 = -349kJ/mol, ΔH3 = -381kJ/mol
Hence, ΔH = 120-349-381 = -610kJ/mol
On the basis of the following thermochemical data
The value of enthalpy of formation of OH- ion at 25ºC is -
The correct answer is option A
Adding eqn(1)&(2), we have
Hence the value of enthalpy of formation of OH− ion at 25℃ is −228.88kJ.
In a fuel cell methanol is used as fuel and oxygen gas is used as an oxidizer. The reaction is
At 298 K standard Gibb's energies of formation for CH3OH(l), H2O(l) and CO2(g) are -166.2, -237.2 and -394.4 kJ mol-1 respectively. If standard enthalpy of combustion of methanol is -726 kJ mol-1, efficiency of the fuel cell will be-
CH3OH (l) + 3/2 O2 (g) → CO2 (g) + 2H2O(l)
∆Gr = ∆Gf(CO2,g) + 2∆Gf(H2O,l) - ∆Gf(CH3OH,l) - 3/2∆Gf(O2,g)
= -394.4 + 2(-237.2) - (-166.2) - 0
= -702.6 kJ
%age efficiency = 702.6/726 × 100 = 97%
The value of enthalpy change (DH) for the reaction C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l)
at 27°C is -1366.5 kJ mol-1. The value of internal energy change for the above reaction at this temperature will be -
The correct answer is option B
The change in the number of moles of gaseous species Δn = 2−3 =−1
ΔH = ΔE+ΔnRT
−1366.5 kJ/mol = ΔE+[(−1)×8.314×10−3 kJ/mol/K×(27+273) K]
ΔE = −1364.0 kJ/mol
The value of internal energy change for the reaction is −1364.0 kJ/mol.
Consider the reaction :
4NO2(g) + O2(g) → 2N2O5(g), ΔrH = -111kJ If N2O5(s) is formed instead of N2O5(g) in the above reaction, the ΔrH value will be : (given, ΔH of sublimation for N2O5 is 54 kJ mol-1)
The correct answer is Option D.
From Hess’s Law;
ΔHf + ΔHsub = ΔHreaction
ΔHf = ΔHreaction - ΔHsub
= - 111 kJ - 54 kJ
= - 165 kJ
Thus the enthalpy of the formation (ΔHf) for N2O5(s) is -165 kJ
In view of the signs of DrG° for the following reactions :
PbO2 + Pb → 2 PbO, DrG° < 0
SnO2 + Sn → 2 SnO, DrG° > 0,
which oxidation states are more characteristic for lead and tin ?
The standard enthalpy of formation of NH3 is -46.0 kJ mol-1 . If the enthalpy of formation of H2 from its atoms is -436 kJ mol-1 and that of N2 is -712 kJ mol-1 , the average bond enthalpy of N - H bond in