1

### NEET 2013 (Karnataka)

When 5 litres of a gas mixture of methane and propane is perfectly combusted at 0oC and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed, The amount of heat released from this combustion in kJ ($\Delta$Hcomb. (CH4) = 890 kJ mol$-$1, $\Delta$Hcomb. (C3H8) = 2220 kJ mol$-$1) is
A
38
B
317
C
477
D
32

## Explanation

CH4 + 2O2 $\to$ CO2 + 2H2O

C3H8 + 5O2 $\to$ 3CO2 + 4H2O

CH4 + C3H8 = ${5 \over {22.4}} = 0.22$ moles.

${O_2} = {{16} \over {22.4}} = 0.71$ moles

$2x + (0.22 \times x)5 = 0.71$

x = 0.13

Heat liberated = 0.13 $\times$ 890 + 0.09 $\times$ 2220 = 316 kJ
2

### NEET 2013

A reaction having equal energies of activation for forward and reverse reactions has
A
$\Delta$H = 0
B
$\Delta$H = $\Delta$G = $\Delta$S = 0
C
$\Delta$S = 0
D
$\Delta$G = 0

## Explanation

For a general reaction,

ΔH = Activation energy of forward reaction – Activation energy of backward reaction.

As, both the energies of activation have same value thus, ΔH = 0.

$\Delta$G is not equal to zero because if it is so the reaction must be in equilibrium which is not in this case
3

### AIPMT 2012 Prelims

The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0oC is
A
10.52 cal/(mol K)
B
21.04 cal/(mol K)
C
5.260 cal/(mol K)
D
0.526 cal/(mol K)

## Explanation

H2O($l$) → H2O(s)

∆H = 1.435 Kcal/mol

T = 0 + 273K = 273K

$\Delta S = {{\Delta H} \over T}$

$\Rightarrow$ $\Delta S = {{1.435} \over {273}}$ = 5.26 $\times$ 10-3 kcal/mol K

$\Rightarrow$ $\Delta S$ = 5.260 cal/mol K
4

### AIPMT 2012 Prelims

Standard enthalpy of vaporisation $\Delta$vapHo for water at 100oC is 40.66 kJ mol$-$1. The internal energy of vaporisation of water at 100oC (in kJ mol$-$1) is
A
+37.56
B
$-$43.76
C
+ 43.76
D
+ 40.66

## Explanation

H2O(l) $\buildrel {100^\circ \,C} \over \longrightarrow$ H2O(g)

∆Ho = 40.66kJ mol–1

∆Ho = ∆uo + $\Delta$ng RT

$\Delta$ng = 1, R = 8.314 × 10–3 kJ mol–1 k–1

T = 100 + 273 = 373 K

$\Rightarrow$ 40.66 = ∆uo + (1) (8.314 × 10–3) × 373

$\Rightarrow$ ∆uo = 37.56 kJ mol–1