The decomposition of XY is second order in XY and has a rate constant of 7.06×10−3 M−1⋅s−1 at a certain temperature.
PART A
If the initial concentration of XY is 0.160 M , how long will it take for the concentration to decrease to 6.80×10−2 M ?
Express your answer using two significant figures.
PART B
If the initial concentration of XY is 0.050 M, what is the concentration of XY after 45.0 s ?
Express your answer using two significant figures.
PART C
If the initial concentration of XY is 0.050 M, what is the concentration of XY after 550 s ?
Express your answer using two significant figures.
1/[A] = 1/[A0] + Kt
K = 7.06×10−3 M−1⋅s−1
part-A
1/[A] = 1/[A0] + Kt
K = 7.06×10−3 M−1⋅s−1
[A0] = 0.16M
[A] = 6.8*10^-2 M = 0.068M
1/0.068 = 1/0.16 + 7.06*10^-3 * t
14.7 = 6.25 + 7.06*10^-3 * t
14.7-6.25 = 7.06*10^-3 * t
8.45 = 7.06*10^-3 * t
t = 8.45/(7.06*10^-3) = 1196.88sec>>>>answer
part-B
1/[A] = 1/[A0] + Kt
K = 7.06×10−3 M−1⋅s−1
[A0] = 0.05M
t = 45s
1/[A] = 1/0.05 + 7.06*10^-3*45
1/[A] = 20 + 0.3177
1/[A] = 20.3177
[A] = 1/20.3177 = 0.049M
part-C
1/[A] = 1/[A0] + Kt
K = 7.06×10−3 M−1⋅s−1
[A0] = 0.05M
t = 500s
1/[A] = 1/0.05 + 7.06*10^-3*500
1/[A] = 20 + 3.53
1/[A] = 23.53
[A] = 1/23.53 = 0.043M
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