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. 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? 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. Rate expression -rA = k CA. CB

= k CA^2 (For same concentrations of both the reactants)

Where k= rate constant

if value of k is constant for particular or assumed order. then asumed order of reaction is correct.

Order is assumed first based on that k is calculated, if value of k is constant then asumed order is correct. if not then change the order and get equal k.

2) for every 10 deg C rise in temperature reaction rate doubles or value of rate constant doubles.

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