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1

### AIPMT 2010 Mains

Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be
A
infinite
B
3 Joules
C
9 Joules
D
zero

## Explanation

Since the ideal gas expands spontaneously into vacuum,, Pext = 0.

$$\therefore$$ Work done is also zero.
2

### AIPMT 2010 Mains

Match List I (Equations) with List II (Type of processes) and select the correct option.

List I List II
Equations Type of processes
A. Kp > Q (i) Non- spontaneous
B. $$\Delta$$Go < RT ln Q (ii) Equilibrium
C. Kp = Q (iii) Spontaneous and
endothermic
D. T > $${{\Delta H} \over {\Delta S}}$$ (iv) Spontaneous
A
A - (i), B - (ii), C - (iii), D - (iv)
B
A - (iii), B - (iv), C - (ii), D - (i)
C
A - (iv), B - (i), C - (ii), D - (iii)
D
A - (ii), B - (i), C - (iv), D - (iii)

## Explanation

When Kp > Q, rate of forward reaction > rate of backward reaction.

$$\therefore$$ Reaction is spontaneous.

When $$\Delta$$Go < RT ln Q, $$\Delta$$Go is positive, reverse reaction is feasible, thus reaction is non spontaneous.

When Kp = Q, rate of forward reaction > rate of backward reaction.

$$\therefore$$ Reaction is in equilibrium.

When T$$\Delta$$S > $$\Delta$$H, $$\Delta$$G will be negative only when $$\Delta$$H = +ve.

$$\therefore$$ Reaction is spontaneous and endothermic.
3

### AIPMT 2010 Prelims

Standard entropies of X2, Y2 and XY3 are 60, 40 and 50 J K$$-$$1 mol$$-$$1 respectively. For the reaction

1/2X2 + 3/2Y2 $$\rightleftharpoons$$ XY3, $$\Delta$$H = $$-$$ 30 kJ,

to be at equilibrium, the temperature should be
A
750 K
B
1000 K
C
1250 K
D
500 K

## Explanation

Given reaction is :

$${1 \over 2}$$X2 + $${3 \over 2}$$Y2 ⇌ XY3

We know,

$$\Delta$$So = $$\sum {S_{products}^o} - \sum {S_{reac\tan ts}^o}$$

= 50 - (30 + 60) = -40 J K-1 mol-1

At equilibrium $$\Delta$$Go = 0

$$\Delta$$Ho = T$$\Delta$$So

$$\therefore$$ $$T = {{\Delta {H^o}} \over {\Delta {S^o}}}$$ = $${{ - 30 \times {{10}^3}} \over { - 40}}$$ = 750 K
4

### AIPMT 2010 Prelims

For an endothermic reaction, energy of activation is Ea and enthalpy of reaction is $$\Delta$$H (both of these in kJ/mol). Minimum value of Ea will be
A
less than $$\Delta$$H
B
equal to $$\Delta$$H
C
more than $$\Delta$$H
D
equal to zero

## Explanation

Here,

Ea = activation energy of forward reaction

E’a = activation energy of backward reaction

$$\Delta$$H = enthalpy of the reaction From the given diagram it is clear that

Ea = E’a + $$\Delta$$H

$$\therefore$$ Ea > $$\Delta$$H

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