Question

In: Chemistry

The rate constant for a certain reaction is k = 1.90×10−3 s−1 . If the initial...

The rate constant for a certain reaction is k = 1.90×10−3 s−1 . If the initial reactant concentration was 0.850 M, what will the concentration be after 15.0 minutes? A zero-order reaction has a constant rate of 2.80×10−4 M/s. If after 75.0 seconds the concentration has dropped to 9.00×10−2 M, what was the initial concentration?

A zero-order reaction has a constant rate of 2.80×10−4M/s. If after 75.0 seconds the concentration has dropped to 9.00×10−2M, what was the initial concentration?

Solutions

Expert Solution

K    = 2.303/t log[A0]/[A]

K    = 1.9*10^-3sec^-1

[A0]   = 0.85M

t          = 15minutes   = 15*60    900sec

K    = 2.303/t log[A0]/[A]

1.9*10^-3   = 2.303/900 log0.85/[A]

log0.85/[A]     = 1.9*10^-3*900/2.303

log0.85/[A]     = 0.743

0.85/[A]     = 10^0.743

0.85/[A]     = 5.5335

[A]              = 0.85/5.5335    = 0.154M

zero ordr

K   = 2.8*10^-4sec

t     = 75sec

[A]t = 9*10^-2M   = 0.09M

Kt   = [A]t - [A]0

2.8*10^-4*75 = 0.09-[A]0

0.021            = 0.09-[A]0

-[A]0             = 0.021-0.09

[A0]             = 0.069M


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