We will now consider reaction mixture 5. Calculate the molar concentrations of e
ID: 483058 • Letter: W
Question
We will now consider reaction mixture 5. Calculate the molar concentrations of each reactant as done in problem 2. Use the concentrations for Mixture 5 you just calculated, along with the orders of the reaction (m, n, and p. from problem 3), and the average rate constant (problem 4), to solve Eq. 2 for rate. This is a prediction of how long it will take for the l_2 color to disappear from your mixture. Rate = k[acetone]^m[H*]^n[I_2)^p Predicted Rate:_ To find the predicted time, recall rate = [I_2]_o/time. Use the rate from problem 5 and the molar concentration of (l_2)_o from problem 5 to solve for the predicted time. Predicted time for reaction __ secondsExplanation / Answer
5.
4.0 M acetone
1.0 M HCl
0.0050 M I2
H2O
Volume (mL)
10.0
5.0
10.0
25.0
Concentration (M)
0.8
0.1
0.001
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Total volume of solution = (10.0 + 5.0 + 10.0 + 25.0) mL = 50.0 mL.
Use the dilution law to find out the concentrations:
M1*V1 = M2*V2 where M1 = concentration of concentrated solution; V1 = volume of concentrated solution; M2 = concentration of diluted solution and V2 = volume of diluted solution.
Acetone:
(4.0 M)*(10.0 mL) = M2*(50.0 mL)
===> M2 = 4.0*10.0/50.0 M = 0.8 M
HCl:
(1.0 M)*(5.0 mL) = M2*(50.0 mL)
===> M2 = 1.0*5.0/50.0 M = 0.1 M
I2:
(0.0050 M)*(10.0 mL) = M2*(50.0 mL)
===> M2 = 0.0050*10.0/50.0 M = 0.001 M
6. Need to know the values of m, n and p and the average rate constant to answer this question.
7. Need to know the rate of the reaction from problem 6 to answer the question.
4.0 M acetone
1.0 M HCl
0.0050 M I2
H2O
Volume (mL)
10.0
5.0
10.0
25.0
Concentration (M)
0.8
0.1
0.001
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