In the first-order reaction A --> Products, the initial concentration of A is 1.56 M and the concentration is 0.869 M after 48.0 min. What is the value of the rate constant, k ?
A. 3.84 X 10-2 min-1
B. 2.92 X 10-2 min-1
C. 5.68 X 10-2 min-1
D. 1.22 X 10-2 min-1
show steps pleaseeeee!
A. 3.84 X 10-2 min-1
B. 2.92 X 10-2 min-1
C. 5.68 X 10-2 min-1
D. 1.22 X 10-2 min-1
show steps pleaseeeee!
-
ln[f] = = -kt + ln[i]
f = final
i = initial
k = constant
t = time
ln[0.869] = -k(48.0min) + ln[1.56]
-0.140412 = -k(48.0min) + 0.444686
-0.5850978 = -k(48min)
-0.5850978 / 48min = -k
-0.0121895 = -k
k = 0.0121895
k = 1.22 x 10^-2
Any more questions just let me know. I'd be glad to help!
4th of July and I'm at home bored!
Goodluck
f = final
i = initial
k = constant
t = time
ln[0.869] = -k(48.0min) + ln[1.56]
-0.140412 = -k(48.0min) + 0.444686
-0.5850978 = -k(48min)
-0.5850978 / 48min = -k
-0.0121895 = -k
k = 0.0121895
k = 1.22 x 10^-2
Any more questions just let me know. I'd be glad to help!
4th of July and I'm at home bored!
Goodluck