16.1.1 Order of Reaction

• What is the order of reaction with respect to a reactant defined as?

  Power in rate equation
• The overall order of a reaction is the sum of the orders with respect to each reactant
• The overall order of a reaction is calculated by multiplying the individual orders of reactants.

  False
• If $\text{Rate} =$$k[A]^{2}[B]^{0}$, what is the overall order of the reaction?


  2
• Match the order of reaction with its effect on reaction rate when concentration doubles:

  Zero Order ↔️ No change in rate

  First Order ↔️ Rate doubles

  Second Order ↔️ Rate quadruples
• A zero-order reaction proceeds at a constant rate, regardless of reactant concentration
• The rate of a first-order reaction is halved when the reactant concentration is halved.
• What is the rate equation for a zero-order reaction?

  $\text{Rate} =$$k$
• The decomposition of ammonia on a platinum surface is an example of a zero-order reaction
• The order of reaction indicates how the reaction rate changes with changes in the volume of reactants.

  False
• How is the overall order of a reaction calculated?

  Sum of individual orders
• Match the term with its definition:

  Order of Reaction ↔️ Power in rate equation

  Rate Equation ↔️ Relates rate to concentrations

  Overall Order ↔️ Sum of individual orders
• In a zero-order reaction, the rate doubles when the reactant concentration doubles.

  False
• The rate of a first-order reaction is directly proportional to the concentration of the reactant
• What does the order of reaction determine?

  How reaction rate changes
• In a first-order reaction, the rate doubles when the concentration doubles.
• What is the characteristic of a zero-order reaction regarding reactant concentration?

  Independent of concentration
• What type of reaction has a rate directly proportional to the concentration of the reactant?

  First-order reaction
• What happens to the rate of a second-order reaction if the reactant concentration is doubled?

  It quadruples
• Zero-order reactions occur at a constant rate regardless of reactant concentration.
• Match the order of reaction with its characteristic:

  Zero Order ↔️ Constant rate

  First Order ↔️ Rate proportional to [A]

  Second Order ↔️ Rate proportional to [A]^{2}
• Give an example of a zero-order reaction.

  Decomposition of ammonia on platinum
• What is the rate equation for a first-order reaction?

  $\text{Rate} =$$k[A]$
• In a first-order reaction, the rate doubles when the reactant concentration doubles.
• Give an example of a first-order reaction.

  Radioactive decay of polonium-210
• In a second-order reaction, the rate quadruples when the concentration doubles.
• What is an example of a second-order reaction?

  Reaction between NO and ozone
• Steps to determine the order of reaction experimentally using the method of initial rates:

  1️⃣ Vary reactant concentrations

  2️⃣ Measure initial rates

  3️⃣ Compare rate changes with concentration changes

  4️⃣ Solve rate equation for the exponent
• First-order reactions yield straight lines when $\ln[A]$ is plotted against time.
• If doubling the concentration of a reactant quadruples the reaction rate, what is the order of the reaction with respect to that reactant?

  Second order
• What three variables are plotted against time to determine the order of a reaction using the graphical method?

  $[A]$, $\ln[A]$, $\frac{1}{[A]}$
• A reaction is second order with respect to reactant A
• The order of reaction indicates how the reaction rate changes with changes in reactant concentration.
• What is the overall order of a reaction if $m =$$2$ and $n =$$1$?


  3
• There are three primary types of reaction orders: zero order, first order, and second order.
• Match the order of reaction with its effect on the rate of reaction.

  Zero Order ↔️ Rate is independent of concentration.

  First Order ↔️ Rate doubles when concentration doubles.

  Second Order ↔️ Rate quadruples when concentration doubles.
• Zero-order reactions proceed at a constant rate regardless of reactant concentration.
• What is an example of a zero-order reaction?

  Decomposition of ammonia on platinum
• The rate equation for a first-order reaction is $\text{Rate} =$$k[A]$, where $[A]$ is the concentration of the reactant.
• The half-life of a first-order reaction is constant and depends only on the rate constant.