Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Joules23 on February 01, 2008, 04:47:37 PM
-
--------------------
7) A compound decomposes by a first-order reaction. The concentration of compound decreases from 0.1124 M to 0.0905 M in 5.2 min. What fraction of the compound remains after 7.6 min?
Using the first order integration law i got K=6.946e-4 (used 312sec for t)
Then again i used integrated law to find [A] and i used 456 sec for t..
I got [A]=.08189
When it asks "What fraction of the compound remains .." do i just
[A]/.1124 = remaining fraction?
.08189/.1124 =.7285 ???
-------------------
10) Experimental data for the reaction below have been plotted in the following three different ways (with concentration units in mol/L).
A 2 B + C
(http://www.webassign.net/zumchem/zumchem6_e12-35.gif)
(a) What is the concentration of A after 7 s?
.0125 M
(b) What are the first three half-lives for this experiment?
first half-life
s
second half life
s
third half-life
s
I need help with part (b).. This is what im doing
t1/2=1/([A]ok)
k=slope=10
[A]o for first reaction = (1/20)= .05
1/(.05x10) = 2 .. but thats incorrect?
-------------
-
7 is correct. 10a is correct.
For 10b, your calculation for [A]o is wrong. You calculated the concentration of A when t=1. You want [A] when t=0.
-
Okkkk.. so first half life.. [A]o = (1/10)=.1
second half life.. [A]o = (1/20)=.05
third half life..[A]o = (1/30)=.0333..
plug those values into the second order half life formula?
-
Third half life [A]o is wrong. After one half life, you have 1/2 left. After two half lives, you have (1/2)*(1/2) = 1/4 left.