In Part IA of the experiment, your first mixture (Mixture will be made from the

Question

In Part IA of the experiment, your first mixture (Mixture will be made from the following reactants, with water as the solvent: 10.0 mL 4.0 M acetone 10.0 mL 1.0 M HCl 10.0 mL 0.0050 M 20.0 mL H20 Use the dilution formula (CIV C2V2) to calculate the initial concentrations of acetone, H (from HC), and iodine (L2) in the reaction mixture. Show your work, and place your answers below. TYou can also fill in the boxes in Table 1B.] [acetone] M; [12] M; Using the reaction mixture in Problem 1, a student found that it took 320 seconds for the color of the to disappear. Remember: initial means the initial concentration of a component in the mixture at the start of the reaction. a. What was the rate of the reaction? Hint: rate- rate b. Write the rate law for the reaction as it would apply to the mixture. (Fill in numbers and units for the rate and concentrations of each reactant). Rate c. What are the unknowns that remain in the equation in Part b? #7 Rates

Explanation / Answer

Total volume of the mixture = 10mL + 10mL +10mL +20mL = 50mL

[acetone] = C(initial) * V(initial)/total volume = 4M *10mL/50mL = 0.8 M

[H+] = C(initial) * V(initial)/total volume = 1M *10mL/50mL = 0.2 M

[I2] = C(initial) * V(initial)/total volume = 0.005M*10mL/50mL = 0.001 M

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rate = [I2]/t = 0.001M/320s = 3.13*10^-6 M/s

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rate = k[0.8]^m[0.2]^n[I2]^p

3.13*10^-6 M/s = k[0.8]^m[0.2]^n[I2]^p

unknown are : k = rate constant, m = order with respect to acetone, n = reaction order wrt H+ and p= order wrt I2

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