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This quiz contains 10 questions from a mix of 1 subtopics.
What is the term for the time taken for the reactant concentration to decrease to half of its initial value?
rate constant
Boltzmann distribution
half-life
activation energy
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The results above are obtained for the rate of reaction, A + B ➔ C.
What is the rate equation?
rate = k[A]2[B]
rate = k[A][B]
rate = k[A]2[B]2
rate = k[A][B]2
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The rate equation for a reaction is rate = k[X]2[Y]. The initial rate of reaction is 5.4 x 10-4 mol dm-3 s-1 and the initial concentrations of X and Y are 0.010 mol dm-3 and 0.20 mol dm-3 respectively.
Calculate the value of k.
mol-2 dm6 s-1
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The decomposition of nitrous oxide, N2O, is first order with respect to N2O:
2N2O(g) ➔ 2N2(g) + O2(g)
N2O has a half-life of 100 s.
What is the value of the rate constant, k?
144 s-1
3.01 x 10-3 s-1
332 s-1
6.93 x 10-3 s-1
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In the iodine clock reaction, what is the initial rate of reaction proportional to?
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In an iodine clock reaction, the concentration of iodide ions is varied and the time taken for the solution to turn blue (t) is measured. The reaction is first order with respect to I-(aq).
Sketch the shape of the graph below.
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In an iodine clock reaction, the concentration of iodide ions is varied, and the time taken for the solution to turn blue (t) is measured. The rate equation is given by rate = k[I-(aq)]. The graph of t1 against [I-(aq)] is plotted above.
Using the graph, calculate the value of the rate constant, k. Give your answer to 2 significant figures.
s-1
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What type of reaction produces the concentration-time graph shown above?
zero order
first order
second order
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What type of reaction produces the rate-concentration graph shown above?
zero order
second order
first order
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What type of reaction produces the rate-concentration graph shown above?
second order
zero order
first order
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