Chemistry · Elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units
Which of the following statement is true for the reaction, The rate law is \left
Which of the following statement is true for the reaction, \( \boldsymbol{H}_{2}+\boldsymbol{B} \boldsymbol{r}_{2} \rightarrow \boldsymbol{2} \boldsymbol{H} \boldsymbol{B} \boldsymbol{r} \) The rate law is \( \frac{\boldsymbol{d} \boldsymbol{x}}{\boldsymbol{d} \boldsymbol{t}}=\boldsymbol{k}\left[\boldsymbol{H}_{2}\right]\left[\boldsymbol{B} \boldsymbol{r}_{2}\right]^{1 / 2} \)
- A. order of reaction is 1.5
- B. molecularity of the reaction is 2
- C. by increasing the concentration of \( B r_{2} \) four times the rate of reaction is doubled
- D. all the above are correct
Step-by-step solution
A: Order = sum of exponents (1 + 1/2) = 1.5, true. B: Molecularity of the overall reaction is 2 from stoichiometric coefficients, true. C: Rate ∝ [Br₂]^{1/2}; fourfold increase in [Br₂] doubles rate, true. Hence all three statements are correct.
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