Rate equation is rate = k[MnO4-]x[H2C2O4]y Understand what [MnO4-], [H2C2O4], x, y and k are. How to calculate the x,y, and k in this experiment?
2Mno4-+5H2C2O4+6H+2Mn2++10CO2+8H2O
we cannot predict the directly x and y by looking at the reaction
we need the experimental data to find these values means
;ike at different concentrations of MnO4 how the how the oxalic acid varied?
so please provide that data
i know this is a third order reaction
here x = 2 nad y = 1
Rate = k[MnO4-]2 [H2C2O4]1
now from your data put all the rate constant and concentrations you will get the K value
Rate equation is rate = k[MnO4-]x[H2C2O4]y Understand what [MnO4-], [H2C2O4], x, y and k are. How...
1. Determine which reactant is limiting the rate of
reaction. Justify the answer.
2. Determine the rate of reaction in trial 1,2,3
3. What are the experimental values for n and m?
Thank you so so much for your help.
Experiment: Reaction Kinetics Aim: To find the reaction orders and rate constants for the following reaction: 3 H2C2O4(aq) + 2 MnO4 (aq) --> 6 CO2+ 2 OH(aq) + 2 H2O + 2 MnO2s In other words to obtain m, n,...
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what is the E° for the equation H2O2+MnO4 - ------>O2+Mn 2+ and how can E° be calculated for any other equation?
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A solution of 5 x 10-3 M MnO4- is dissolved in 25.00 mL of H2O. What volume of H2O must be added to the solution to reduce the concentration of [MnO4- ] to 7.5 x 10-4 M? If possible, please show work so I can learn and understand how you approached the problem and solved it. Thanks!
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What is this balanced equation?
MnO4−(aq) +
I−(aq) I2(s) +
MnO2(s)
I got 2MnO4-(aq) +
6I-(aq) +
4H2O(l) ⇌ 3I2(s)
+ 2MnO2(s) + 8OH-(aq)
but webassign is saying it's wrong.
edit: nevermind, figured it out. 2
MnO4-(aq) + 8
H+(aq) +
6I-(aq) ⇌ 3
I2(s) + 2 MnO2(s) + 4
H2O(l)
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