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Questions 17 - 18:
Hsub3AsOsub4 + 3I^- + 2Hsub3O^+ -> Hsub3AsOsub3 + Isub3^- + 3Hsub2O
The oxidation of iodide ions by arsenic acid in acidic aqueous solution occured accoring to the balanced equation above. The experimental rate law for the reaction at 25 degree C is:
17) What is the order of the reaction with respect to I^-?
18) According to the rate law for the reaction an increase in concentration of the Hydronium has what effect on the reaction at 25 degree C?
a) the rate of reaction increases
b) the rate of reaction decreases
c) the value of the equilibrium constant increases
d) the value of the equilibrium constant decreases
e) neither the rate nor the value of the equilibrium constant is changed
The rate law for the reaction : k [Hsub3AsOsub4] [I^-]^3 [Hsub3O]^2
17) The order with respect to I^- is first ...
The answer is given succinctly in approximately 50-100 words.