Medium
Consider the following reactions:
$A$ $\rightarrow P_1; B$ $\rightarrow P_2; C$ $\rightarrow P_3; D$ $\rightarrow P_4$
The orders of the above reactions are $a, b, c,$ and $d,$ respectively. The following graph is obtained when $\log[\text{rate}]$ vs. $\log[\text{conc.}]$ are plotted:
Among the following,the correct sequence for the order of the reactions is:
$A$ $\rightarrow P_1; B$ $\rightarrow P_2; C$ $\rightarrow P_3; D$ $\rightarrow P_4$
The orders of the above reactions are $a, b, c,$ and $d,$ respectively. The following graph is obtained when $\log[\text{rate}]$ vs. $\log[\text{conc.}]$ are plotted:
Among the following,the correct sequence for the order of the reactions is:
- A$a > b > c > d$
- B$c > a > b > d$
- C$d > b > a > c$
- D$d > a > b > c$
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For a hypothetical reaction $A + B + C \rightarrow \text{Product}$,the rate is given by $r = -\frac{d[A]}{dt} = K[A]^{1/2}[B]^{1/3}[C]^{1/4}$. The order of the reaction is:
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$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.
Consider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:
$[A_2]_0$ $[B_2]_0$ Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ $0.1 \ M$ $0.1 \ M$ $2.5 \times 10^{-4}$ $0.2 \ M$ $0.1 \ M$ $5.0 \times 10^{-4}$ $0.2 \ M$ $0.2 \ M$ $1.0 \times 10^{-3}$
The value of the rate constant for the above reaction is:
| $[A_2]_0$ | $[B_2]_0$ | Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $2.5 \times 10^{-4}$ |
| $0.2 \ M$ | $0.1 \ M$ | $5.0 \times 10^{-4}$ |
| $0.2 \ M$ | $0.2 \ M$ | $1.0 \times 10^{-3}$ |
The value of the rate constant for the above reaction is:
DifficultTS EAMCET 2024
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