Reaction mixture-1:
[BrO3-](mixture) :
Since KBrO3 is completely dissociated, [BrO3-](mixture) = [KBrO3]
V(mixture) = (Volume of all reactants in reaction flask-1) + (Volume of all reactants in reaction flask-2)
= 10+10+10+10+10 = 50 mL (Same for all reaction mixture)
V(stock) = 10 mL
[BrO3-](stock) = 0.010 M (Please confirm whether it is 0.010 M or 0.040 M as the 2nd figure is unclear)
Hence [BrO3-](mixture) = (0.010 M * 10 mL] / 50 mL = 0.0020 M
[H+](mixture):
Since HCl is completely dissociated, [H+](mixture) = [HCl](mixture)
V(mixture) = 50 mL
V(stock) = 10 mL
[H+](stock) = 0.10 M
=> [H+](mixture) = (0.10 M * 10 mL] / 50 mL = 0.020 M
Similarly we can calculate for rest of the reaction mixture as:
Reaction mixture-2:
[I-](mixture) = (0.010 M * 20 mL] / 50 mL = 0.0040 M
[BrO3-](mixture) = (0.010 M * 10 mL] / 50 mL = 0.0020 M
[H+](mixture) = (0.10 M * 10 mL] / 50 mL = 0.020 M
Reaction mixture-3:
[I-](mixture) = (0.010 M * 10 mL] / 50 mL = 0.0020 M
[BrO3-](mixture) = (0.010 M * 20 mL] / 50 mL = 0.0040 M
[H+](mixture) = (0.10 M * 10 mL] / 50 mL = 0.020 M
Reaction mixture-4:
[I-](mixture) = (0.010 M * 10 mL] / 50 mL = 0.0020 M
[BrO3-](mixture) = (0.010 M * 10 mL] / 50 mL = 0.0020 M
[H+](mixture) = (0.10 M * 20 mL] / 50 mL = 0.040 M
Reaction mixture-5:
[I-](mixture) = (0.010 M * 8 mL] / 50 mL = 0.0016 M
[BrO3-](mixture) = (0.010 M * 5 mL] / 50 mL = 0.0010 M
[H+](mixture) = (0.10 M * 15 mL] / 50 mL = 0.030 M
how do you find them? im a bit lost. this is what we used A. Dependence...
need help with relative rate problems
Experiment 21 Data and Calculations: Rates of Chemical Reactions, Il. A Clock Reaction A. Dependence of Reaction Rate on Concentration Reaction: 61(ag + BrO,ag)+ 6H(aq)3aqp+ Brap+HO0 rate irBeO, Tr-- In all the reaction mistures used in this experiment, the color change occurred when a constant predetermined aumber of moles of BrO," had been used n in the reaction The color "clock" allows you to measue the ime mgaired for this fixed number of moles...
can you help me make sure of m,n,p values.
LILAC Rection Name Section Experiment 16 Data and Calculations: Rates of Chemical Reactions, H. A Clock Reaction (1) so A. Dependence of Reaction Rate on Concentration Reaction: 6 l'(aq) + Bro, (aq) + 6 Haq) +31(aq) + Br(aq) + 3H,0 rale ("BO, Hy A(Bro, In all the reaction mixtures used in the experiment, the color change curred when number of moles of Bro, had been used up by the reaction. The...
This is a better photo
Section Name 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 2 by mixing 20 ml. 0.010 M KI. 10 mL 0.0001 M Na.S.0. 10 mL 0.040 M KBrO and 10 ml, O.10 M HCT using the procedure given. It took about 45 seconds for the color to turn bluc. She found the concentrations of...
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...
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...
A student studied the clock reaction described in this experiment. She set up Reaction Mixture 2 by mixing 20 mL 0.010 M KI, 10 mL .001 M Na2S2O3, 10 mL .040 M KBrO3, and 10 mL 0.10 M HCl using the procedure given. It took 45 seconds for the color to turn to blue. a. She found the concentration of each reactant in the reacting mixture by realizing that the number of moles of each reactant did not change when...
how do I calculate the isolated moles and molarity
of the 0.2M
KIO3?
0.1 M Sulfuric Distilled Solution A Mixturel Mixture II Mixture III Mixture IV 0.20 M KIO3 Solution 5 mL 5 mL 10 mL 10 mL Acid 0 mL 0.5 mL 0 mL 0.5 mL water 15 ml 14.5mL 10 mL 9.5 mL Lalculations: I. (6pt) Calculate the total number of moles of iodate ion present in each 0.2 M KlO3 solution. Calculate the molarity of iodate ion...
Data and Calculations: Determination of the Equilibrium Constant for a Chemical Reaction Method II Volume in mL 2.00 x 103 M Fe(NO) Volume in mL, Depth in mm Volume in ml. 2.00 x 103 M Method I Mixture Unknówn KSCN Water Absorbance Standard FESCNP 4mL 1 5.00 x 10 M 1,00 .227 3mL 2 5,00 202 x 10 M 2,00 90 x 10 M .304 3 5,00 3.00 2mL 955 x 104 M I ImL 4 5.00 4,00 19x 10...
Learning Goal: To calculate average and relative reaction rates. You can measure the rate of a reaction, just like you can measure the speed a jogger runs. While a jogger would be reported to run a specific number of miles in an hour, miles/hour, a reaction is reported to form product or consume reagent in molar concentration per second, M/s. Reaction rate can be defined either as the increase in the concentration of a product per unit time or as...
Please help me solve page 2
and 3
Data Table 1 Mixture 4 Mixture1 Mixture 2 Mixture 3 Volume of 4.00M Acetone (C3H6O) Volume of 1.0OM HCI Volume of 0.00500M I Volume of H20 10.0ml 20.0mL 10.0mL 10.0mL 10.0mL 20.0mL 10.0mL 10.0mL 5.0mL 10.0ml 10.0mL 10.0mL 10.0mL 25.0mL 10.0mL 20.0mL 50.0mL 50.0mL Total Volume (mL) 50.0mL 50.0mL ec 2.07m4.2 sec 2-24 mi21344s 24-8 5%0 4-51 mine 270-66e 241 218K-24-852 Reaction Time (s) 24-65C 24 850C Mixture Temperature (°C) Concentration and...