Difficult
Consider the following data for the given reaction $2 HI_{(g)} \rightarrow H_{2_{(g)}} + I_{2_{(g)}}$. The order of the reaction is:
Experiment $1$ $2$ $3$ $[HI] \ (mol \ L^{-1})$ $0.005$ $0.01$ $0.02$ Rate $(mol \ L^{-1} \ s^{-1})$ $7.5 \times 10^{-4}$ $3.0 \times 10^{-3}$ $1.2 \times 10^{-2}$
| Experiment | $1$ | $2$ | $3$ |
|---|---|---|---|
| $[HI] \ (mol \ L^{-1})$ | $0.005$ | $0.01$ | $0.02$ |
| Rate $(mol \ L^{-1} \ s^{-1})$ | $7.5 \times 10^{-4}$ | $3.0 \times 10^{-3}$ | $1.2 \times 10^{-2}$ |
- A$1$
- B$2$
- C$3$
- D$4$
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$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$
Initial $[A_2]$ Initial $[B_2]$ $R.O.R. (r) \ M s^{-1}$ $0.2$ $0.2$ $0.04$ $0.1$ $0.4$ $0.04$ $0.2$ $0.4$ $0.08$
Order of reaction with respect to $A_2$ and $B_2$ are respectively:
| Initial $[A_2]$ | Initial $[B_2]$ | $R.O.R. (r) \ M s^{-1}$ |
|---|---|---|
| $0.2$ | $0.2$ | $0.04$ |
| $0.1$ | $0.4$ | $0.04$ |
| $0.2$ | $0.4$ | $0.08$ |
Order of reaction with respect to $A_2$ and $B_2$ are respectively:
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