Concept explainers
(a)
Interpretation:
The given reaction is to be shown as second order using the given data.
Concept introduction:
The rate law/rate equation for a
(b)
Interpretation:
The rate constant of reaction should be determined.
Concept introduction:
For second order reaction:
Where, k is rate constant, t is time, [A]t is concentration of A at time t and [A]o is the concentration of A at initial time that is at t = 0.
(c)
Interpretation:
Time at which [ArSO2H] is equal to 0.05 M should be determined.
Concept introduction:
In a second order
(d)
Interpretation:
Time at which [ArSO2H] is equal to 0.025 M should be determined.
Concept introduction:
In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.
(e)
Interpretation:
Time at which [ArSO2H] is equal to 0.035 M should be determined.
Concept introduction:
In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.
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General Chemistry: Principles and Modern Applications (11th Edition)
- The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)arrow_forwardFor the first-order reaction N2O5 (g) —> 2NO2 (g) + l/2O2(g), T_I/2 = 22.5 h at 20C and 1.5h at 40C respectively. (1) Calculate the value ofthe activation energy in kJ • mol^-1;(2) Ifthe Arrhenius constant A = 2.05 x 10^13 s^-1, determine the value ofk at 30C.arrow_forwardChlorine atoms react with methane, forming HCl and CH3. The rate constant for the reaction is 6.00 × 107 M–1 s–1 at 298 K. The experiment was repeated at three other temperatures, resulting in the following data: Calculate the the activation energy for the reaction in kJ/molarrow_forward
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