224. In one liter of a solution containing two strong acids HBr and $\text{HBrO}_4$, the concentration of each is $0.01$ mol per liter. The reaction: $$\text{HBrO}_4(\text{aq}) + 5\text{HBr}(\text{aq}) \rightarrow 3\text{Br}_2(\text{l}) + 3\text{H}_2\text{O}(\text{l})$$ with rate law: $\text{rate} = k[\text{BrO}_4^-][\text{Br}^-][\text{H}^+]^2$, is carried out. By adding $0.09$ mol $\text{HBr}(\text{g})$ to this solution (without changing the volume), at the start of the reaction, the rate of the reaction compared to the initial state is how many times? (1) $5 \times 1/\Delta$ (2) $211/\Delta$ (3) $3 \times 7/\Delta$ (4) $312/\Delta$
\textbf{224.} In one liter of a solution containing two strong acids HBr and $\text{HBrO}_4$, the concentration of each is $0.01$ mol per liter. The reaction:
$$\text{HBrO}_4(\text{aq}) + 5\text{HBr}(\text{aq}) \rightarrow 3\text{Br}_2(\text{l}) + 3\text{H}_2\text{O}(\text{l})$$
with rate law: $\text{rate} = k[\text{BrO}_4^-][\text{Br}^-][\text{H}^+]^2$, is carried out. By adding $0.09$ mol $\text{HBr}(\text{g})$ to this solution (without changing the volume), at the start of the reaction, the rate of the reaction compared to the initial state is how many times?
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(1) $5 \times 1/\Delta$ \quad (2) $211/\Delta$ \quad (3) $3 \times 7/\Delta$ \quad (4) $312/\Delta$
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