1. When you calculated k in the rate equation for the reaction of KMnO, solution
ID: 1082231 • Letter: 1
Question
1. When you calculated k in the rate equation for the reaction of KMnO, solution and HO, 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, solution and H2C2Os 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. 2. 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. 3. Consider the reaction that occurs when a CIO, solution and a solution containing hydroxide ions (OH) are mixed at 0 °C, shown in Equation 18. 2CIO2 (aq) + 2 OH' (aq) CIO' (aq) + Clor (aq) + H2O(l) Eq. 18Explanation / Answer
Solution:
The rate constant depends on the temperature according to this equation also calle arrhenius equation.
k = A*exp(-Ea/RT)
A is a constant
-Ea is the activation energy which is a constant number
R is gas constant
T is temperature
So the assumption that you have to make in order to find k experimentally by changing the concentration of the solutions is that the solutions are always at the same temperature (The temperature from the lab is constant)
B) Yes It may be practical as long as the temperature remains constant
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