When you calculated k in the rate equation for the reaction of KMnO_4 solution a

Question

When you calculated k in the rate equation for the reaction of KMnO_4 solution and H_2C_2O_4 solution, you assumed k had the same value under the conditions of determinations 1, 2, and 3. (a) What assumption did you make about the reaction of KMnO_4 solution and H_2C_2O_4 solution in those determinations that allowed you to consider k to be a constant? (b) Would it be sound practice to compare the results of determinations 4-6 when calculating k? Briefly explain. Do your experimental data substantiate the rule of thumb regarding the effect on the reaction rate of a 10-degree increase in reaction temperature? Briefly explain. Consider the reaction that occurs when a ClO_2 solution and a solution containing hydroxide ions (OH^- are mixed at 0 degree C, shown in Equation 18. 2ClO_2 (aq) + 2 OH^-(aq) rightarrow ClO_3^- (aq) + ClO_2^-(aq) + H_2O(l)

Explanation / Answer

1/ For determinationof rate of the reaction,

a. The concentration remains unaffected by mixing the given volume of compounds. Thi give a rate constant as same.

b. A 10 oC increase in reaction enhances the kinetic energy of reactants and thus collision between the molecules is greater which gives higher rate of reaction. This is supported by the reaction data.

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