1
MHT CET 2023 10th May Morning Shift
+1
-0

The reaction, $$3 \mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_3^{-}+2 \mathrm{Cl}^{-}$$ occurs in two steps:

i. $$\quad 2 \mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_2^{-}+\mathrm{Cl}^{-}$$

ii. $$\quad \mathrm{ClO}_2^{-}+\mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_3^{-}+\mathrm{Cl}^{-}$$,

the reaction intermediate is:

A
$$\mathrm{Cl}^{-}$$
B
$$\mathrm{ClO}_2^{-}$$
C
$$\mathrm{ClO}_3^{-}$$
D
$$\mathrm{ClO}^{-}$$
2
MHT CET 2023 9th May Evening Shift
+1
-0

Calculate the rate constant of first order reaction if the concentration of the reactant decreases by $$90 \%$$ in 30 minutes.

A
$$7.7 \times 10^{-2}$$ minute $$^{-1}$$
B
$$4.2 \times 10^{-2}$$ minute $$^{-1}$$
C
$$2.1 \times 10^{-2}$$ minute $$^{-1}$$
D
$$3.5 \times 10^{-2}$$ minute $$^{-1}$$
3
MHT CET 2023 9th May Evening Shift
+1
-0

The rate law for the reaction $$\mathrm{A}+\mathrm{B} \rightarrow$$ product is given by rate $$=k[A][B]$$ Calculate $$[A]$$ if rate of reaction and rate constant are $$0.25 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$$ and $$6.25 \mathrm{~mol}^{-1} \mathrm{dm}^3 \mathrm{~s}^{-1}$$ respectively $$\left[[\mathrm{B}]=0.25 \mathrm{~mol} \mathrm{dm}^{-3}\right]$$

A
$$0.22 \mathrm{~mol} ~\mathrm{dm}^3$$
B
$$0.16 \mathrm{~mol} ~\mathrm{dm}^3$$
C
$$0.30 \mathrm{~mol} ~\mathrm{dm}^3$$
D
$$0.25 \mathrm{~mol} ~\mathrm{dm}^3$$
4
MHT CET 2023 9th May Evening Shift
+1
-0

Find the average rate of formation $$\mathrm{O}_{2(\mathrm{~g})}$$ in the following reaction.

\begin{aligned} & 2 \mathrm{NO}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \\ & {\left[-\frac{\Delta[\mathrm{NO}]}{\Delta \mathrm{t}}\right]=x \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}} \end{aligned}

A
$$\frac{\mathrm{x}}{2} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$$
B
$$x \mathrm{~mol} ~\mathrm{dm}^{-3} \mathrm{~s}^{-1}$$
C
$$2 x~ \mathrm{mol} ~\mathrm{dm}^{-3} \mathrm{~s}^{-1}$$
D
$$4 x ~\mathrm{mol} ~\mathrm{dm}^{-3} \mathrm{~s}^{-1}$$
EXAM MAP
Medical
NEET