Question:Write the net ionic balanced equation for the reaction of bromate with bromide with hydrogen ions that produces bromine and water.
Using the following experimental data:
Run [BrO3^-] (M) [Br^-] (M) [H+] (M) Initial Rate (M/sec)
1 0.100 0.100 0.100 8.09 x10^-4
2 0.200 0.100 0.100 1.61 x10^-3
3 0.200 0.200 0.100 3.17 x10^-3
4 0.100 0.100 0.200 3.28 x10^-3
a. What is the order with respect to each reactant and the overall order?
b. What is the rate constant?
c. What is the complete rate law for this reaction?
d. Most reactions exhibit different rates for the individual reactants and products based on stoichiometry. Which of those multiple rates does the term "rate of reaction" refer to?
e. What is the rate of disappearance of hydrogen ion at the concentration when[BrO3^-] = 0.350 M, [Br-] = 0.150 M, and [H+]= 0.100 M?
f. What is the rate of disappearance of hydrogen ion at the concentrations given in part (e)?