Change in enthalpy for reaction
2H2O2(l) → 2H2O(l) + O2 (g)
if heat of formation of H2O2(l) and H2O(l) are -188 and -286 kJ/mol respectively is,
-196 kJ/mol
+ 196 kJ/mol
+ 948 kJ/mol
-948 kJ/mol
The enthalpy of combustion of H2, cyclohexene (C6H10) and cyclohexane (C6H12) are - 241, -3800 and -3920 kJ per mol respectively. Heat of hydrogenation of cyclohexene is
- 121 kJ per mol
+ 121 kJ per mol
+ 242 kJ per mol
- 242 kJ per mol
If ΔE is the heat of reaction for
C2H5OH(I) + 3O2(g) → 2CO2 (g) + 3H2O(I)
at constant volume, the ΔH (heat of reaction at constant pressure), then the correct relation is
ΔH = ΔE + RT
ΔH = ΔE - RT
ΔH = ΔE - 2RT
ΔH = ΔE + 2RT
Unit of entropy is
JK-1 mol-1
J mol-1
J-1 K-1 mol-1
JK mol-1
The absolute enthalpy of neutralisation of the reaction
MgO(s) + 2HCI(aq) → MgCI2(aq) + H2O(l) will be
less than -57.33 kJ mol-1
-57.33 kJ mol-1
greater than -57.33 kJ mol-1
57.33 kJ mol-1
Identify the correct statement for change of Gibb's energy for a system (ΔGsystem ) at constant temperature and pressure.
If ΔGsystem > 0, the process is spontaneous
If ΔGsystem = 0, the system has attained equilibrium
If ΔGsystem = 0, the system is still moving in a particular direction
If ΔGsystem< 0, the process is not spontaneous
Considering entropy (S) as a thermodynamic parameter, the criterion for the spontaneity of any process is
Ssystem + Ssurrounding > 0
Ssystem - Ssurrounding > 0
Ssystem > 0 only
Ssurrounding > 0 only
The correct relationship between free energy and equilibrium constant K of a reaction is
Go = - RT In K
G = RT In K
Go = RT In K
G = - RT In K
If ΔH is the change in enthalpy and ΔE, the change in internal energy accompanying a gaseous reaction, then
ΔH is always greater than ΔE
ΔH < ΔE only if the number of moles of products is greater than the number of moles of the reactants.
ΔH is always less than ΔE
ΔH < ΔE only if the number of moles of products is less than the number of moles of the reactants
Consider the following reaction occurring in an automobile
2C8H18(g) + 25O2(g) → 16 CO2(g) + 18 H2O(g)
The sign of ΔH, ΔS, and ΔG would be
+, -, +
-, +, -
-, +, +
+, +, -
