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adoni [48]
3 years ago
5

It is found that a gas undergoes a first-order decomposition reaction. If the rate constant for this reaction is 8.1 x 10-2 /min

, how long will it take for the concentration of the gas to change from an initial concentration of .1M to 1.0 x 10-2 M?
Chemistry
1 answer:
kap26 [50]3 years ago
3 0

Answer:

28.43 min

Explanation:

Using integrated rate law for first order kinetics as:

[A_t]=[A_0]e^{-kt}

Where,  

[A_t] is the concentration at time t

[A_0] is the initial concentration

Given that:

The rate constant, k = 8.1\times 10^{-2} min⁻¹

Initial concentration [A_0] = 0.1 M

Final concentration [A_t] = 1.0\times 10^{-2} M

Time = ?

Applying in the above equation, we get that:-

1.0\times 10^{-2}=0.1e^{-8.1\times 10^{-2}\times t}

0.1e^{-8.1\times \:10^{-2}t}=10^{-2}

e^{-8.1\times \:10^{-2}t}=\frac{1}{10}

\ln \left(e^{-8.1\times \:10^{-2}t}\right)=\ln \left(\frac{1}{10}\right)

t=28.43\ min

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You can also learn about molarity from the following question:

brainly.com/question/14782315

#SPJ4

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