DP Chemistry Questionbank

• Syllabus

Topic 16: Chemical kinetics

Sub sections and their related questions

16.1 Rate expression and reaction mechanism

• 15M.1.hl.TZ1.20: Which statement about a first-order reaction is correct? A.     The reactant concentration...
• 15M.1.hl.TZ1.21: Consider the rate expression: \[{\text{Rate}} = k{\text{[X][Y]}}\] Which change decreases the...
• 15M.1.hl.TZ2.20: What are the units of the rate constant for a zero-order reaction? A.     s B.    ...
• 15M.1.hl.TZ2.21: The hydrolysis of tertiary bromoalkanes with a warm dilute aqueous sodium hydroxide solution...
• 15M.2.hl.TZ1.7c.i: Determine the orders of reaction of the reactants and the overall rate expression for the...
• 15M.2.hl.TZ1.7c.ii: Determine the rate constant, \(k\), with its units, using the data from experiment 3.
• 15M.2.hl.TZ1.7c.iii: Identify the molecularity of the rate-determining step in this reaction.
• 15M.2.hl.TZ2.2c.i: Identify the rate-determining step.
• 15M.2.hl.TZ2.2c.ii: A student hypothesized that the order of reaction with respect to \({{\text{H}}_{\text{2}}}\) is...
• 14M.1.hl.TZ1.20: X and Y react according to the equation \({\text{2X}} + {\text{Y}} \to {\text{Z}}\). The reaction...
• 14M.1.hl.TZ2.21: Which combination shows a second-order rate expression with the correct rate constant units?
• 14M.2.hl.TZ1.2b: State the rate expression for this reaction.
• 14M.2.hl.TZ1.2c: Determine the value of the rate constant, \(k\), and state its units.
• 14M.2.hl.TZ1.2d: State an equation for a possible rate-determining step for the reaction.
• 14M.2.hl.TZ2.6a: (i)     State the volumes of the liquids that should be mixed. (ii)     State why it is...
• 14M.2.hl.TZ2.6b: (i)     Deduce the rate expression of this mechanism.     (ii)     The results of an...
• 14N.1.hl.TZ0.20: Consider the following reaction between nitrogen monoxide and...
• 14N.2.hl.TZ0.11c: (i)     In some reactions, increasing the concentration of a reactant does not increase the rate...
• 14N.2.hl.TZ0.11d: Sketch a graph of rate constant \((k)\) versus temperature.
• 13N.1.hl.TZ0.21: The following experimental rate data were obtained for a reaction carried out at temperature...
• 13N.1.hl.TZ0.22: Consider the following proposed two-step reaction mechanism at temperature T.      Step 1:    ...
• 13N.2.hl.TZ0.8e.ii: State the rate expression for this reaction and the units of the rate constant.
• 13M.1.hl.TZ1.20: For the gas phase reaction: \[{\text{A(g)}} + {\text{B(g)}} \to {\text{C(g)}}\] the...
• 13M.1.hl.TZ1.21: Which graph best represents a second-order reaction?
• 13M.2.hl.TZ1.9c.i: Deduce the order of reaction with respect to...
• 13M.2.hl.TZ1.9c.ii: Deduce the rate expression.
• 13M.2.hl.TZ1.9c.iii: Based on the rate expression obtained in (c) (ii) state the units of the rate constant, \(k\).
• 13M.1.hl.TZ2.20: Experimental data shows that a reaction in which Y is a reactant is first order with respect to...
• 13M.1.hl.TZ2.21: Which statement about a reaction best describes the relationship between the temperature, \(T\),...
• 13M.1.hl.TZ2.22: Carbon monoxide and nitrogen dioxide react to form carbon dioxide and nitrogen monoxide according...
• 13M.2.hl.TZ2.2b: State how the rate constant, k , varies with temperature, T.
• 13M.2.hl.TZ2.2c: Determine the activation energy, \({E_{\text{a}}}\), correct to three significant figures and...
• 12N.2.hl.TZ0.6c: (i)     Concentration of reactant X against time for a zero-order reaction. (ii)     Rate of...
• 12N.2.hl.TZ0.6d: (i)     Deduce the rate expression. (ii)     Determine the rate constant, \(k\), and state its...
• 10N.1.hl.TZ0.20: Consider the following reaction. \[{\text{2P}} + {\text{Q}} \to {\text{R}} + {\text{S}}\] This...
• 10N.2.hl.TZ0.5g: (i)     Deduce the rate expression for the reaction. (ii)     Determine the value of the rate...
• 09N.2.hl.TZ0.6a.i: State the rate expression for the forward reaction.
• 09N.2.hl.TZ0.6b: Consider the following...
• 10M.2.hl.TZ1.2b: (i)     Deduce the order of reaction for each substance and the rate expression from the...
• 10M.2.hl.TZ1.2c: Using the data from Experiment 1, determine the concentration of the substances used and the rate...
• 10M.1.hl.TZ2.21: The following data were obtained for the reaction between gases A and B. Which relationship...
• 09M.1.hl.TZ2.21: Consider the following...
• 09M.1.hl.TZ2.22: The rate expression for a reaction is: \[{\text{rate}} = k{\text{[X][Y]}}\] Which statement is...
• 09M.1.hl.TZ2.23: Consider the following reaction...
• 09M.2.hl.TZ2.7b.i: The kinetics of the reaction were studied at this temperature. The table shows the initial rate...
• 09M.2.hl.TZ2.7b.ii: Deduce the rate expression for the reaction.
• 09M.2.hl.TZ2.7b.iii: Determine the value of the rate constant for the reaction from Experiment 3 and state its units.
• 09M.2.hl.TZ2.7c.i: Identify the rate-determining step.
• 09M.2.hl.TZ2.7c.ii: Identify the intermediate involved in the reaction.
• 11M.1.hl.TZ1.21: Bromine and nitrogen(II) oxide react according to the following...
• 11M.1.hl.TZ1.23: Which step is the rate-determining step of a reaction? A.     The step with the lowest...
• 11M.2.hl.TZ1.2c: The rate expression for this reaction is rate...
• 11M.1.hl.TZ2.21: The rate information below was obtained for the following reaction at a constant...
• 11M.1.hl.TZ2.22: Consider the following...
• 11M.2.hl.TZ2.3b.ii: Deduce the units for the rate constant \(k\).
• 12M.1.hl.TZ2.19: Which graph represents a reaction that is second order with respect to X for the reaction X...
• 11N.1.hl.TZ0.22: Which graph represents a reaction that is first order with respect to reactant A.
• 11N.2.hl.TZ0.8e.ii: The table below shows initial rates of reaction for different concentrations of each reactant for...
• 11N.2.hl.TZ0.8f.i: Identify the intermediate in the reaction.
• 11N.2.hl.TZ0.8f.ii: The observed rate expression is...
• 11N.2.hl.TZ0.8g: The following two-step mechanism has been suggested for the reaction of...
• 16M.1.hl.TZ0.21: The data shows the effect of...
• 16M.1.hl.TZ0.22: Which pair of graphs...
• 16M.2.hl.TZ0.3a: (i) State the equation for the overall reaction. (ii) Deduce the rate expression consistent with...
• 16N.1.hl.TZ0.21: Which statement describes the characteristics of a transition state relative to the potential...
• 16N.1.hl.TZ0.22: Decomposition of hydrogen peroxide in an aqueous solution proceeds as follows. 2H2O2(aq) →...
• 16N.2.hl.TZ0.3e: (i) Using the graph, explain the order of reaction with respect to sodium thiosulfate. (ii) In a...
• 17M.1.hl.TZ1.20: The table gives rate data for the reaction in a suitable solvent. C4H9Br + OH− → C4H9OH +...
• 17M.1.hl.TZ1.21: What are the units for the rate constant, k, in the expression? Rate = k [X]2[Y] A.     mol2...
• 17M.2.hl.TZ1.1b: The student then carried out the experiment at other acid concentrations with all...
• 17M.2.hl.TZ1.1c: When the concentration of iodine is varied, while keeping the concentrations of acid and...
• 17M.2.hl.TZ1.1d: When the reaction is carried out in the absence of acid the following graph is...
• 17M.1.hl.TZ2.12: Which is the first step in the CFC-catalysed destruction of ozone in UV light? A.     CCl2F2 →...
• 17M.1.hl.TZ2.21: Which is correct about reaction mechanisms? A.     A species that is zero order does not take...
• 17M.2.hl.TZ2.5b.i: State the rate expression for the reaction.
• 17M.2.hl.TZ2.5b.ii: The following mechanism is proposed for the...
• 17M.2.hl.TZ2.5b.iii: State one method that can be used to measure the rate for this reaction.
• 17M.2.hl.TZ2.5b.v: Sketch the relationship between the rate of reaction and the concentration of NO2.
• 17N.1.hl.TZ0.21: The rate expression for the reaction X (g) + 2Y (g) → 3Z (g) is  rate = k[X]0 [Y]2 By which...
• 17N.1.hl.TZ0.22: Which pair of statements explains the increase in rate of reaction when the temperature...
• 17N.2.hl.TZ0.2e.i: Deduce the order of reaction with respect to Cl2 and NO.
• 17N.2.hl.TZ0.2e.ii: State the rate expression for the reaction.
• 17N.2.hl.TZ0.2e.iii: Calculate the value of the rate constant at 263 K.
• 18M.1.hl.TZ1.19: What are correct labels for the Maxwell−Boltzmann energy distribution curves?
• 18M.1.hl.TZ1.20: The reaction between NO2 and F2 gives the following rate data at a certain temperature. What...
• 18M.2.hl.TZ1.4b.iv: Deduce the rate expression for the reaction.
• 18M.2.hl.TZ1.4b.v: Calculate the rate constant of the reaction, stating its units.
• 18M.1.hl.TZ2.20: When X reacts with Y to give Z, the following graph is plotted. What can be deduced from the...
• 18M.1.hl.TZ2.21: Which statement is correct? A.     The value of the rate constant, k, is independent of...

16.2 Activation energy

• 14M.1.hl.TZ1.21: The rate constant for a reaction is determined at different temperatures. Which diagram...
• 14M.2.hl.TZ1.2e: Suggest how the activation energy, \({E_{\text{a}}}\), for this reaction may be determined.
• 14N.1.hl.TZ0.21: What happens to the rate constant, k, and the activation energy, \({E_{\text{a}}}\), as the...
• 13N.2.hl.TZ0.1f.i: State the labels for each axis.   x-axis:   y-axis:
• 13N.2.hl.TZ0.1f.ii: Use the graph to determine the activation energy of the reaction, in...
• 13M.2.hl.TZ1.3b: Use the graph on page 8 to determine the value of the activation energy, \({E_{\text{a}}}\), in...
• 13M.2.hl.TZ1.3c: On the graph on page 8, sketch the line you would expect if a catalyst is added to the reactants.
• 12N.2.hl.TZ0.6e.iii: The rate of this reaction was measured at different temperatures and the following data were...
• 10N.1.hl.TZ0.21: What happens when the temperature of a reaction increases? A.     The activation energy...
• 09N.1.hl.TZ0.21: The activation energy of a reaction may be determined by studying the effect of a particular...
• 09N.2.hl.TZ0.6d: Consider the following graph of \(\ln k\) against \(\frac{1}{T}\) for the first order...
• 09M.2.hl.TZ2.7d.iv: Calculate the activation energy, \({E_{\text{a}}}\), for the reaction, using Table 1 of the Data...
• 11M.2.hl.TZ1.2a: State how the rate constant, \(k\) varies with temperature,\(T\).
• 11M.2.hl.TZ1.2b: Determine the activation energy, \({E_{\text{a}}}\), for this reaction.
• 12M.2.hl.TZ2.9c: (i)     The Arrhenius equation is shown in Table 1 of the Data Booklet. Identify the symbols...
• 11N.2.hl.TZ0.8h: HI(g) decomposes into \({{\text{H}}_2}{\text{(g)}}\) and \({{\text{I}}_{\text{2}}}{\text{(g)}}\)...
• 16M.1.hl.TZ0.23: Which of the terms in...
• 17M.1.hl.TZ2.20: Which is true of an Arrhenius plot of \(\ln k\) (y-axis) against \(\frac{1}{T}\)? A.     The...
• 17M.2.hl.TZ2.5c: The Arrhenius equation, \(k = A{e^{ - \frac{{Ea}}{{RT}}}}\), gives the relationship between the...
• 17N.1.hl.TZ0.22: Which pair of statements explains the increase in rate of reaction when the temperature...
• 18M.1.hl.TZ1.21: What is the effect of increasing temperature on the rate constant, k?  A.     The rate constant...
• 18M.2.hl.TZ1.4d: Describe how the activation energy of this reaction could be determined.
• 18M.2.hl.TZ2.6d: The rate constant for a reaction doubles when the temperature is increased from 25.0 °C to 35...