A)The reaction of mercury(II) chloride with oxalate ion 2 HgCl2 + C2O42-2 Cl- +
ID: 973111 • Letter: A
Question
A)The reaction of mercury(II) chloride with oxalate ion 2 HgCl2 + C2O42-2 Cl- + Hg2Cl2 + 2 CO2 is first order in HgCl2 and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
In an experiment to determine the rate law, the rate constant was determined to be 1.33×10-4 M-1s-1. Using this value for the rate constant, the rate of the reaction when [NO2] = 3.08 M and [F2] = 0.783 M would be
C)
In an experiment to determine the rate law, the rate of the reaction was determined to be 9.38×10-2 Ms-1 when [NO] = 3.19×10-2 M and [O3] = 2.47×10-2 M. From this experiment, the rate constant is .
Explanation / Answer
A. Now that we know that the overall order is third, and the HgCl2 is first, the rate of reaction would be:
rate = k[HgCl2][C2O42-]2
B. rate = k[NO2][F2]
If k = 1.33x10-4 L/mol s then the rate:
rate = 1.33x10-4 * 3.08 * 0.783
rate = 3.21x10-4 M/s
C. rate = k[NO][O3]
k = rate / [NO][O3]
k = 9.38x10-2 / (0.0319)(0.0247)
k = 119.05 L/mol s
Hope this helps