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The rate constant for this first‑order reaction is 0.740 s − 1 0.740 s−1 at 400 ∘ C. 400 ∘C. A ⟶ products A⟶products How long, in seconds, would it take for the concentration of A A to decrease from 0.790 M 0.790 M to 0.230 M? 0.230 M?

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lublana

Answer:

1.668 S

Step-by-step explanation:

We are given that

[tex]A\rightarrow[/tex]Product

For first order reaction,

[tex]t=\frac{1}{k}ln\frac{A_0}{A}[/tex]

[tex]t=\frac{2.303}{k}log\frac{A_0}{A}[/tex]

Rate constant=k=[tex]0.740s^{-1}[/tex]

Temperature=[tex]T=400^{\circ}[/tex]

We have to find the time taken by the reaction when concentration of A to decrease from 0.790 M to 0.230 M.

[tex]A_0=0.79 M[/tex]

[tex]A=0.230[/tex]

Substitute the values then we get

[tex]t=\frac{2.303}{0.740}log\frac{0.79}{0.23}[/tex]

[tex]t=1.668 s[/tex]

Hence, it would take 1.668 s for the concentration of  A to decrease from 0.790 M to 0.230 M.

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