Answer Happy

does someone else know how to do it?
0.8 2011, 2009 Cengage Leaming Data and Calculations: The Iodination of Acetone A. Reaction Rate Data Volume in mL 4.0M Acetone Mixture I II III IV Mixture 10 10 III IV 5 30 Volume in mL 1.0M HCI 10 10 30 10 0.80 M 11M)014/0.50 0.40M 0.40m 2.4m Volume in mL 0.0050 M1₂ W 10 20 10 5 0.20 M 0.20M 450 O.COM 0.20 M Volume in ml. H₂O 20 to 5 127 137 131, 78 B. Determination of Reaction Orders with Respect to Acetone, H* Ion, and 1₂ ratek(acetone)" (1₂)" (H*)" (Eq. 3) Calculate the initial concentrations of acetone, H* ion, and 1₂ in each of the mixtures you studied. Use Equation 5 to find the rate of each reaction. M₁ V₁ (4M (0,052)= M₁ V₁ = M₂ V₂ V₂ (Acetone) (H*) 199 190 208 Time for Reaction in sec 2nd run 1st run 3.10 7:50 7:23 2:12 2:11 24 24 0:43 1:01 (12)0 0.0010 M 0.002 M 0.001 M 0.0005M 3:28 24 23 Temp in "C Rate= (1₂) avg time 50110- 19x6-6 7x10.0 1X10's Substituting the initial concentrations and the rate from the table above, write Equation 3 as it would apply to Reaction Mixture II: x 22 6 Rate II = -4X10 M/S = K (0.80M)" (0.002 m)" (0.201) Now write Equation 3 for Reaction Mixture I, substituting concentrations and the calculated rate from the table: Rate I == 5x10 m/s = K[0.80m)(0.0010M)^(0.20m)
Divide the equation for Mixture II by the equation for Mixture I; the resulting equation should have the ratio of Rate II to Rate I on the left side, and a ratio of acetone concentrations raised to the power m on the right. It should be similar in appearance to Equation 6. Put the resulting equation below: Rate II 4X10M/5 = Rate I = (0.80m/0.80m) 0.8=1" m=0.8=1 Honelosis bag bos 1 0 == 5X10 M/S The only unknown in the equation is m. Solve for m. Now write Equation 3 as it would apply to Reaction Mixture III and as it would apply to Reaction Mixture IV: Rate III = k Rate IV= Using the ratios of the rates of Mixtures III and IV to those of Mixtures II or I, find the orders of the reaction with respect to H* ion and 1₂: Rate III -7x10 m/s =k(0.4mm (0.001m)^ (0.6MY IX 10 M/S = K(2.4) (0.0005) ^ (0.2) P ン Rate Rate IV Rate Mixture SA en of teqst C. Determination of the Rate Constant k Given the values of m, p, and n as determined in Part B, calculate the rate constant k for each mixture by simply substituting those orders, the initial concentrations, and the observed rate from the table into Equation 3.. -- III p=_ ob not to colissima 11 IV Average