Aspirin, C
9
H
8
O
4
, slowly decomposes at room temperature by reacting with water in the atmosphere to produce acetic acid, HC
2
H
3
O
2
, and 2-hydro
x
ybenzoic acid, C
7
H
6
O
3
(this is why old bottles of aspirinoften smell like vinegar):C
9
H
8
O
4
+ H
2
O
p
HC
2
H
3
O
2
+ C
7
H
6
O
3
Concentration and rate data for this reaction are given below
.
[C
9
H
8
O
4
] (M) [H
2
O] (M) Rate (M/s)
0
.
0
1
00 0
.
02002
.
4
v
1
0
±
1
3
0
.
0
1
00 0
.
08009
.
6
v
1
0
±
1
3
0
.
0200 0
.
02004
.
8
v
1
0
±
1
3
W
rite the rate law for this reaction and calculate k (be sure to include the correct units)
1 answer
I must be honest and say this is the most confusing problem I've ever seen and it isn't because of the problem but the way it is posted. Why not write acetic acid as HC2H3O2?
1 answer