Here is information that you will need to help me solve my poblem:
C. (Given the values for m,p,and n caculate the rate constant k for each mixtureby simply substituting those orders, the initial concentrations, and the observed rate from the table....)so I did that and got:
Mixture
k
I= 2.23x10^(-4)
II= 1.56x10^(-4)
III= 4.38x10^(-4)
IV= 2.73x10^(-4)
Average All the number above added together and divided by 4)=
2.725x10^(-4)
E. Time for reaction at about 10 degrees celsius= 150 sec
10 degrees celsius= 283 K
Time for reaction at about 40 degrees celsuis (313 K)= 32 sec
Time for reaction at room temp 25 degrees celsius (298 K)= 143 sec
Based on C and E the problem is:
Calculate the rate constant at each temperature from your data, following the procedure in part C. (note that for E they wanted us to use one reaction mixture- I chose Nr. I)
They give you a chart in which they want you to fill in the Rate, k, lnk and i/((T)x(K)) for 10 C
40 C
room temp
My questions:
Is the rate the time I observed above...150 sec, 32 sec and 143 sec?
Is k the same k for I in part C?
Does T(K) in 1/((T)x(K)) just stand for the temperature in Kalvin?
Is it correct that K would be the same for all three temperatures?
I hope this isn't too much! I have been thinking about this and I am just not sure if what I am thinking is quite right.
3 answers