1
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
$$0.25 \mathrm{~mol} ~\mathrm{dm}^3$$
2
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
$$4 x ~\mathrm{mol} ~\mathrm{dm}^{-3} \mathrm{~s}^{-1}$$
3
MHT CET 2023 9th May Morning Shift
+1
-0

Which from following is the slope of the graph of rate versus concentration of the reactant for first order reaction?

A
$$-\mathrm{k}$$
B
$$\mathrm{k}$$
C
$$\frac{\mathrm{k}}{2.303}$$
D
$$\frac{-\mathrm{k}}{2.303}$$
4
MHT CET 2023 9th May Morning Shift
+1
-0

Calculate the amount of reactant in percent that remains after 60 minutes involved in first order reaction. $$\left(\mathrm{k}=0.02303\right.$$ minute $$\left.^{-1}\right)$$

A
$$25 \%$$
B
$$75 \%$$
C
$$50 \%$$
D
$$12.5 \%$$
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