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

queen_honey_blossom answered 1 year ago

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