Question
In: Chemistry
1. KClO3 decomposes according to the reaction: 2KClO3 → 2KCl + 3O2 If the rate of...
1. KClO3 decomposes according to the
reaction:
2KClO3 → 2KCl + 3O2
If the rate of decomposition of
potassium chlorate at a certain time is determined to be 2.4 x
10-2mol
s-1, what is the
rate of formation of KCl at the same time?
2. The rate law for a reaction involving only A and B is 1st order in A and 4th order in B, respectively. If the concentration of A is increased by a factor of 4 and the concentration of B is tripled the new rate will be:
3. The reaction D ---> products is first order, and the rate constant is 2.7 x 10-4 s-1. If the initial concentration of D is 3.00 M, then what is the final concentration of D after 1.1 hr?
Solutions
Expert Solution
2KClO3 → 2KCl + 3O2
rate of reaction
-
[KClO3]/2t =
+[KCl]/2t
2.4*10-2 /2
= +[KCl]/2t
1.2*10-2
= +[KCl]/2t
+[KCl]/t =
2.4*10-2 mole/sec
2. Rate law
Rate = K[A][B]4
= K*A/4*[3B]4
= K[A][B]4 *81/4
81/4 times increases Or 20.25 ntimes rate inccreases
3. K = 2.303/t*log[A0]/[A]
t = 1.1hr = 1.1*60*60 = 3960 sec
[A0] = 3
K = 2.7*10-4 sec-1
2.7*10-4 = 2.303/3960*log3/[A]
2.7*10-4 = 5.815*10-4 log3/[A]
0.4643 = log3/[A]
2.912 = 3/[A]
[A] = 1.03 M
queen_honey_blossom answered 2 years agoRelated Solutions
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