For trial 1:
Total volume = 10 + 10 + 10 + 10 = 40 mL
[I] = Moles of KI / Total Volume
= 10 mL * 0.01 M of KI / 40 mL
= 0.0025 M
[BrO3] = Moles of KBrO3 / Total Volume
= 10 mL * 0.04 M of KBrO3 / 40 mL
= 0.01 M
[H+] = Moles of HCl / Total Volume
= 10 mL * 0.1 M of HCl / 40 mL
= 0.025 M
Similarly we get the table as shown below for other trials (Row B-D):
|
Trial |
Vol of KI |
Vol of KBrO3 |
Vol of HCl |
[I] |
[BrO3] |
[H+] |
|
1 |
10 |
10 |
10 |
0.0025 |
0.01 |
0.025 |
|
2 |
20 |
10 |
10 |
0.005 |
0.01 |
0.025 |
|
3 |
10 |
20 |
10 |
0.0025 |
0.02 |
0.025 |
|
4 |
10 |
10 |
20 |
0.0025 |
0.01 |
0.05 |
|
5 |
15 |
10 |
10 |
0.00375 |
0.01 |
0.025 |
R = K [I]x [BrO3]y [H+]z
Orders are obtained as:
x = 1.7 ~ 2
y = 2.0 ~ 2
z = 2.26 ~ 2
Rate constant, K as obtained by substituting orders in rate equation as:
K = 1.5 x 1014
How do i get rows B-D order Rate n -Bro,1-t -Hel |Temp. (C) rounded toorder Tria...
how can i get the initial concentration of thiosulfate ion
(S2O3) in reaction mixture 1 ?
and also how can i determine the initial reaction rate for
mixture 1?
A Chemical Clock Your Report: Part I: Determination of the Rate Law 1. Complete Table 1 below using the volumes of each chemical used and the reaction to the reaction times measured that your team used to determine the rate law. Leave any unused rows D Reaction Mixture: Reaction Time /...
rates of chemical reactions
Plz help!! how do I find specific rate constant k, 1/T, In
K
thank you
Rates of Chemical Reactions: Report Form Rate Law Summary: (a) From your measurements, what are the reaction orders with respect to each of the three reactants H;O; HOO (b) What is the rate expression (rate law) for the uncatalyzed reaction? Rate = K LT-] [H202) (c) What is the total reaction order? 2 3. Effect of Temperature on the Reaction Rate...
Experiment 21 Advance Study Assignment: Rates of Chemical Reactions, II. A Clock Reaction 1. A student studied the clock reaction described in this experiment. She set up Reaction Mixture 4 by mixing 10 mL 0.010 M KI, 10 mL 0.001 M Na2S2O3, 10 mL 0.040 M KBrO3, and 20 mL 0.10 M HCl using the procedure given. It took about 21 seconds for the color to turn blue. a. She found the concentrations of each reactant in the reacting mixture...
how do you find them? im a bit lost.
this is what we used
A. Dependence of Reaction Rate on Concentration Reaction: 61aq) + BrO,(aq) + 6H(aq)-31,(aq) + Brtaq) +3H,OD ABrO ABro,THTr rate In all the reaction mixtures used in this experiment, the color change occurred when a constant predetermined number of moles of BrO," had been used up in the reaction. The color "clock" allows you to measure the time required for this fixed number of moles of BrO,...
in
the solvolysis of 2-chloro-2-methylpropane, some di-t-butyo ether
is formed. Explain rhis phenomenon in your own words and show the
reaction sequence that represents this, starting with your starting
materials.
Complete and turn in the problems below. 1. Using an equation like equation 3, derive the expression for k given in equation 4. 2. What solvent mixture are you using in parts A-C? In part D? What effect will the different solvent system used in part D have on the...
just one example/demonstration!
Data needed to be calculated is in highlighted in green boxes.
And I highlighted in red an equation (not sure if thats what you
use to calculate it) And ignore the lab instructions on completeing
a graph!! I already know how to do that in excel, just curious how
Ln (relative rate) and 1/T in K^-1 is calculated by hand*
here is the rest of that lab leading up to the question as I
know its typically...