KINE 505: Seudying the Rate of Reacrion of Porassium Permanganate and Osalic Add
ID: 1026798 • Letter: K
Question
KINE 505: Seudying the Rate of Reacrion of Porassium Permanganate and Osalic Add Post-Laboratory Questions (Use the spaces provided for the answers and additional paper if necessary) (a) Use the method of initial rates to find the order reaction of KMnO, solution and H C204 solution, you of the reaction with respect to CiO2 and with respoct to assumed khad the same value under the conditions of OH Write the rate equation for the reaction of Cioa 1. When you calculated k in the rate equation for the determinations 1, 2, and 3. and OH at o °C. (a) What assumption did you make about the reac- tion of KMnO4 solution and H2C204 solution in those determinations that allowed you to consider k to be a constant? (b) Would it be sound practice to compare the re- suilts of determinations 4-6 when calculating k? Briefly explain. (b) Calculate the rate constant, k, for the reaction of CIO2 and OH at o C 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. (c) Calculate the reaction rate for the reaction CIO2 and OH at O °C when the initial CIO2 and OH con- centrations are 8.25 x 10-3 molL and 5.35 x 10-2 moVL, respectively 3. Consider the reaction that occurs when a Ci02 s0- lution and a solution containing hydroxide ions (OH) are mixed at 0 °C, shown in Equation 18. 2CO2(aq) + 2 OH' (aq) CIOs (ag)+CIO2 (aq)+ H200) (Eq. 18) When solutions containing CIO2 and OH in various concentrations were mixed at 0 °C, the following rate data were obtained: nitial concentration of initial concentration of initial rate for formation of Cio .mobl s determination CIO2 mol/L 1.25 x 10-2 2.50 × 10-2 2.50 x 10-2 number 1.30×10-3 1.30 × 10- 2.60 x 10-3 2.33 x 10-4 9.34 × 10-4 1.87 x 10-3Explanation / Answer
1)
a)
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
2)
Increase in the temperature of a reaction results in the increase in the rate of the reaction.When the temperature is increased by 10 degree C,the rate of the reaction almost doubles.Particles react when they collide.As the temperature increases.Collisions between the particles also increase and thus rate of reaction increases.
When the temperature is increased by 10 degree C Collision frequency will increase.Thus rate of reaction would have been doubled.
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