Writing the Rate Law
Введено| English | Значение |
|---|---|
| rate law/reɪt lɔː/ | закон скорости |
| rate constant/reɪt ˈkɒnstənt/ | константа скорости |
| order/ˈɔːdə/ | порядок реакции |
The formula for speed
- Double a reactant and the speed might double — or quadruple.
- Each reaction has its own sensitivity to concentration.
- A short equation captures exactly how speed depends on amounts.
- But you can only find it by experiment, not by guessing.
The rate law
- The rate law 速率定律 links speed to concentrations:
- Here $k$ is the rate constant 速率常数, and $m$ and $n$ are the orders.
Rate against concentration for zero-, first-, and second-order reactions
The rate constant $k$ changes when the reactant concentrations change.
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False. $k$ depends on temperature (and catalysts), not on concentration; concentrations appear separately in the rate law.
Reaction orders
- The order 反应级数 tells how strongly a concentration affects the rate.
- First order: double $[A]$ and the rate doubles. Second order: double and it quadruples.
- Orders come from experiments, not from the equation's coefficients.
За $\text{rate} = k[A]^2$, doubling $[A]$ multiplies the rate by...
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Second order means $2^2 = 4$ times the rate.
Reaction orders are determined by...
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Orders must be found experimentally, not from coefficients.
A reaction is first order in $[A]$. Tripling $[A]$ changes the rate by a factor of...
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First order means the rate scales directly, so 3 times.
Overall order
- Add the individual orders to get the overall order ($m + n$).
- It sums up the reaction's total sensitivity to concentration.
- The units of $k$ depend on that overall order.
За $\text{rate} = k[A]^2[B]^1$, what is the overall order?
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Overall order $= 2 + 1 = 3$.
For $\text{rate} = k[A]^2[B]$, what happens if you double $[A]$?
- $[A]$ is second order, so doubling it multiplies the rate by $2^2 = 4$.
- The rate quadruples.
Find the reaction order
Use how the rate responds to concentration to find the order in A.
The rate law normally contains only the ____ concentrations, not the products.
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Products usually do not appear in the rate law.
Orders are found by experiment, not read off the balanced equation's coefficients — a very common trap. Only reactants normally appear in the rate law; products usually do not. And the rate constant $k$ changes with temperature but not with concentration.
The rate law $\text{rate} = k[A]^m[B]^n$ links speed to concentrations through the rate constant $k$ and the orders $m$, $n$. Orders come from experiment, not coefficients, and their sum is the overall order. A concentration's order sets how strongly it changes the rate.