The rate law for the reaction $\text{Sucrose} + \text{Water} \xrightarrow{H^+} \text{Glucose} + \text{Fructose}$ is given by:
- A$\text{Rate} = K [\text{sucrose}] [\text{water}]$
- B$\text{Rate} = K [\text{sucrose}] [\text{water}]^0$
- C$\text{Rate} = K [\text{sucrose}]^0 [\text{water}]$
- D$\text{Rate} = K [\text{sucrose}]^{1/2} [\text{water}]^{1/2}$
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Similar Questions
The following are the rate constants of two different reactions. What is the overall order of each reaction?
$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$
$(b)$ $4.5 \times 10^{-3} \ min^{-1}$
$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$
$(b)$ $4.5 \times 10^{-3} \ min^{-1}$
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$NO_{2(g)} + NO_{2(g)} \longrightarrow 2NO_{(g)} + O_{2(g)}$
$NO_{2(g)} + NO_{2(g)} \longrightarrow 2NO_{(g)} + O_{2(g)}$
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