1

### NEET 2017

Mechanism of a hypothetical reaction
X2 + Y2 $\to$ 2XY, is given below :
(i)   X2 $\to$ X + X (fast)
(ii)  X + Y2 $\rightleftharpoons$ XY + Y (slow)
(iii) X + Y $\to$ XY (fast)
The overall order of the reaction will be
A
2
B
0
C
1.5
D
1

## Explanation

Slow step is the rate determining step.

Rate = k[X][Y2] ......(i)

Equilibrium constant for fast step,

K = ${{{{\left[ X \right]}^2}} \over {\left[ {{X_2}} \right]}}$

$\Rightarrow$ [X] = $\sqrt {K\left[ {{X_2}} \right]}$

By substituting [X] in equation (i), we get

Rate = k$\sqrt {K\left[ {{X_2}} \right]}$[Y2] = k' ${{{\left[ {{X_2}} \right]}^{{1 \over 2}}}}$[Y2]

$\therefore$ Order of reaction = ${1 \over 2} + 1$ = 1.5
2

### NEET 2016 Phase 1

The addition of a catalyst during a chemical reaction alters which of the following quantities?
A
Enthalpy
B
Activation energy
C
Entropy
D
Internal energy

## Explanation

A catalyst provides an alternate path to the reaction which has lower activation energy.
3

### NEET 2016 Phase 2

The decomposition of phosphine (PH3) on tungsten at low pressure is a first-order reaction. It is because the
A
rate is proportional to the surface coverage
B
rate is inversely proportional to the surface coverage
C
rate is independent of the surface coverage
D
rate of decomposition is very slow.

## Explanation

At low pressure, rate is proportional to the surface coverage and is of first order while at high pressure it follows zero order kinetic due to complete coverage of surface area.
4

### NEET 2016 Phase 1

The rate of first-order reaction is 0.04 mol L$-$1 s$-$1 at 10 seconds and 0.03 mol L$-$1 s$-$1 at 20 seconds after initiation of the reaction. The half-life period of the reaction is
A
44.1 s
B
54.1 s
C
24.1 s
D
34.1 s

## Explanation

For the first order reaction

A $\to$ Product

Rate $\propto$ [A]

k = ${{2.303} \over {{t_2} - {t_1}}}\log {{{{\left( {rate} \right)}_1}} \over {{{\left( {rate} \right)}_2}}}$

= ${{2.303} \over {20 - 10}}\log {{0.04} \over {0.03}}$

= 0.0287 sec-1

${t_{{1 \over 2}}} = {{0.693} \over k} = {{0.693} \over {0.0287}}$ = 24.14 sec