Consider the following reaction in aqueous solution:
5
Br−(aq)
+
BrO3−(aq)
+ 6
H+(aq)
---> 3
Br2(aq)
+ 3
H2O(l)
i) The equation that relates the rate expressions
for this reaction in terms of the disappearance of Br−,
BrO3− and the formation of Br2 and
H2O is (Choose the correct
letter.):
NOTE: { } is being used to represent the molar
concentration.
A. R = -1/5{ Δ Br - }/ Δ t = -1/1{ Δ BrO 3- }/ Δ t = - 1/6{ Δ H + }/ Δ t = -1/3{ Δ Br 2 }/ Δ t |
B. R = +1/5{ Δ Br - }/ Δ t = +1/1{ Δ BrO 3- }/ Δ t = -1/3{ Δ Br 2 }/ Δ t = +1/3{ Δ H 2 O}/ Δ t |
C. R = -1/5{ Δ Br - }/ Δ t = -1/1{ Δ BrO 3- }/ Δ t = -1/6{ Δ H + }/ Δ t = +1/3{ Δ H 2 O}/ Δ t |
D. R = -1/5{ Δ Br - }/ Δ t = -1/1{ Δ BrO 3- }/ Δ t = +1/3{ Δ Br 2 }/ Δ t = +1/3{ Δ H 2 O}/ Δ t |
E. R = -1/1{ Δ Br - }/ Δ t = -1/5{ Δ BrO 3- }/ Δ t = +1/3{ Δ Br 2 }/ Δ t = +1/3{ Δ H 2 O}/ Δ t |
If the rate of disappearance of Br – ( aq ) at
a particular moment during the reaction is 3.5 x 10
–4M s –1 ,
( NOTE : For
scientific notation, use "E" or "e" to replace "x 10" & do NOT
leave any space between the numbers and letter, e.g., 1.2E3 or
1.1e-4.)
ii) what is the rate of appearance of Br 2 ( aq
) at that moment? (Give answer in scientific
notation): M.s
-1
iii) calculate the overall or average rate of the reaction.
(Give answer in scientific
notation): M.s
-1
I have found parts i and ii but am struggling with part iii. Thanks!
Consider the following reaction in aqueous solution: 5 Br−(aq) + BrO3−(aq) + 6 H+(aq) ---> 3...
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