The correct expression for the rate of reaction given below is:
\(5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})\)

1.	\(\frac{\Delta\left[B r^{-}\right]}{\Delta t}=5 \frac{\Delta\left[H^{+}\right]}{\Delta t} \)	2.	\(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=\frac{6}{5} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \)
3.	\(\frac{\Delta[\mathrm{Br^-}]}{\Delta t}=\frac{5}{6} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \)	4.	\(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=6 \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t}\)

The correct representation of an exothermic reaction is:

1.		2.
3.		4.	Both 1 and 2

Rate law for the reaction \(A+2 B \rightarrow C\) is found to be
Rate = k[A][B]
If the concentration of reactant 'B' is doubled, keeping the concentration of A constant, then the value of the rate of the reaction will  be:

An incorrect statement about the collision theory of chemical reaction is:

A first-order reaction is 50 % completed in 1.26 x 10¹⁴ s. The time required for 100 % completion
of the reaction will be:

1. 1.26 × 10¹⁵ s

2. 2.52 × 10¹⁴ s

3. 2.52 × 10²⁸ s

4. Infinite

An incorrect statement regarding the catalyst is:

Consider the reaction A$\to$B. The concentration of both the reactant and the product varies exponentially with time.

The graph that accurately depicts how reactant and product concentrations change with time is:

1.		2.
3.		4.

The correct graphical representation of first-order reaction is:

(a)		(b)
(c)		(d)

Match the graph given in Column I with the order of reaction given in Column II.
More than one item in Column I may be linked to the same item in Column II:

Column I		Column II
(a)		(a)	1st order
(b)		(b)	Zero order
(c)
(d)

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