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AP Intermediate 2nd Year Chemical Kinetics — practice questions

Explore 89 free Chemical Kinetics questions in AP Intermediate 2nd Year Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Chemical Kinetics questions and exercises with answers

Showing questions 1–30 of 89.

For a first-order reaction, the half-life period $t_{1/2}$ is related to the rate constant $k$ as:Read the answer and worked solution →The units of the rate constant for a zero-order reaction are:Read the answer and worked solution →The SI/CGS-style units of the **rate of a chemical reaction** are:Read the answer and worked solution →For the reaction A → B, the rate of reaction can be written as:Read the answer and worked solution →The **rate constant** $k$ in a rate law equals the rate of reaction when:Read the answer and worked solution →The order of a reaction:Read the answer and worked solution →For a zero-order reaction, the units of the rate constant $k$ are:Read the answer and worked solution →For a first-order reaction, the units of the rate constant $k$ are:Read the answer and worked solution →For the same reaction ($2N_2O_5 \to 4NO_2 + O_2$, $d[N_2O_5]/dt = -0.02$), the **rate of formation of $NO_2$** is:Read the answer and worked solution →If rate = $k[A][B]^2$, what are the units of $k$?Read the answer and worked solution →For the reaction A + B → P with $\text{rate} = k[A][B]^2$, rate = $3.6 \times 10^{-2}$ mol dm⁻³ s⁻¹ when [A] = 0.2 M and [B] = 0.1 M. $k$ equals:Read the answer and worked solution →For the reaction R → P, the *instantaneous* rate of reaction is given by:Read the answer and worked solution →A catalyst on the bench changes:Read the answer and worked solution →For rate = k[A][B]², the overall order is:Read the answer and worked solution →A first-order reaction plots linearly as:Read the answer and worked solution →Half-life of a first-order reaction is:Read the answer and worked solution →Per Arrhenius, raising T:Read the answer and worked solution →For a reaction to proceed, colliding molecules must have:Read the answer and worked solution →A catalyst:Read the answer and worked solution →The RATE CONSTANT ($k$) of a reaction isRead the answer and worked solution →For a FIRST-ORDER reaction with rate constant $k$, the half-life is given byRead the answer and worked solution →For a ZERO-ORDER reaction $A \to \text{products}$, which graph is a STRAIGHT LINE?Read the answer and worked solution →A first-order reaction has a rate constant of $k = 6.93\times 10^{-3}\,\text{s}^{-1}$ at a certain temperature. The half-life is closest toRead the answer and worked solution →NEET · Chemistry · Rate Law — Gap FillRead the answer and worked solution →Rebuild a sample from its halvesRead the answer and worked solution →Order or molecularity?Read the answer and worked solution →True or false: order and molecularityRead the answer and worked solution →Read the order off the rate lawRead the answer and worked solution →Complete the definition of orderRead the answer and worked solution →True or false: where a rate law comes fromRead the answer and worked solution →

Worked practice questions

For a first-order reaction, the half-life period $t_{1/2}$ is related to the rate constant $k$ as:

  1. $t_{1/2} = \dfrac{2.303}{k}$
  2. $t_{1/2} = \dfrac{0.693}{k}$
  3. $t_{1/2} = \dfrac{[A]_0}{2k}$
  4. $t_{1/2} = \dfrac{1}{k[A]_0}$
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Correct answer: B. $t_{1/2} = \dfrac{0.693}{k}$

For a first-order reaction $k = \dfrac{2.303}{t}\log\dfrac{[A]_0}{[A]}$. Setting $[A] = [A]_0/2$ at $t = t_{1/2}$ gives $k t_{1/2} = \ln 2 = 0.693$, hence $t_{1/2} = 0.693/k$. Option B is the zero-order expression option C is the second-order one.

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The units of the rate constant for a zero-order reaction are:

  1. $\text{mol}\,L^{-1}\,s^{-1}$
  2. $L^2\,\text{mol}^{-2}\,s^{-1}$
  3. $L\,\text{mol}^{-1}\,s^{-1}$
  4. $s^{-1}$
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Correct answer: A. $\text{mol}\,L^{-1}\,s^{-1}$

Units of $k$ for an $n$-th order reaction are $\text{mol}^{1-n}\,L^{n-1}\,s^{-1}$. Putting $n=0$ gives $\text{mol}\,L^{-1}\,s^{-1}$, which is the same as the unit of rate itself, since the rate of a zero-order reaction is independent of concentration.

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The SI/CGS-style units of the **rate of a chemical reaction** are:

  1. L mol⁻¹ s⁻¹
  2. mol dm⁻³ s⁻¹
  3. mol L⁻¹
  4. s⁻¹
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Correct answer: B. mol dm⁻³ s⁻¹

Rate = change in concentration / change in time, hence units are concentration/time = mol dm⁻³ s⁻¹ (or mol L⁻¹ s⁻¹).

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