The molar heat capacity 'C' of water at constant pressure is 75 JK-1 mol-1, when 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of water is
4.8 K
6.6 K
1.2 K
2.4 K
If enthalpies of formation of C2H4(g), CO2(g) and H2O(l) at 25oC and 1 atm pressure are 52, -394 and -286 kJ/mol, the enthalpy of combustion of ethene is equal to
-141.2 kJ/mol
-1412 kJ/mol
+14.2 kJ/mol
+1412 kJ/mol
In a closed insulated container a liquid is stirred with a paddle to increase the temperature, which of the following is true ?
E = W ≠ 0, q = 0
E = W = 0, q = 0
E =0,W =q ≠ 0
W =0,E =q ≠ 0
When 1 mole gas is heated at constant volume, temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. Then, which statement is correct ?
q = W = 500 J, E = 0
q = E = 500 J, W = 0
q = - W = 500 J, E = 0
E = 0, q =W = - 500 J
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
The values of ΔH and ΔS for the reaction, C(graphite) + CO2 (g) → 2CO (g) are 170 kJ and 170 JK-1, respectively. This reaction will be spontaneous at
710 K
910 K
1110 K
510 K
From the following bond energies :
H—H bond energy : 431.37 kJ mol-1
C==C bond energy : 606.10 kJ mol-1
C—C bond energy : 336.49 kJ mol-1
C—H bond energy : 410.50 kJ mol-1
Enthalpy for the reaction,
will be
1523.6 kJ mol-1
-243.6 kJ mol-1
-120.0 kJ mol-1
553.0 kJ mol-1
On heating one end of a piece of metal, the other end becomes hot because of
resistance of the metal
mobility of atoms in the metal
energised electrons moving to the other end
minor perturbation in the energy of atoms
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
Given the following entropy values (in JK-1 mol-1) at 298 K and 1 atm : H2(g) : 130.6, CI2(g) : 223.0, HCI(g) : 186.7. The entropy change (in Jk-1 mol-1) for the reaction
H2(g) + CI2(g) → 2HCI(g), is
+ 540.3
+ 727.0
- 166.9
+ 19.8
