Question

In: Chemistry

The following reaction was monitored as a function of time: A→B+C A plot of ln[A] versus...

The following reaction was monitored as a function of time: A→B+C A plot of ln[A] versus time yields a straight line with slope −4.0×10−3 /s .

Part D If the initial concentration of A is 0.220 M , what is the concentration after 230 s ?

[A] = m M

Expert Solution

Answer – We are given reaction, A -----> B + C + A

Graph plot ln[A] versus time yields a straight line with slope −4.0×10⁻³ /s

We know when we draw the graph ln[A] versus time and it gives straight line with negative slope then it is first order of the reaction and the negative slope is equal to the rate constant, k.

So, slope = -k

Rate constant, k = 4.0*10^-3 s^-1

initial concentration [A]o = 0.220 M, time, t = 230 s , [A] = ? M

We know the integrated equation of the first order reaction

ln[A]/[A]o = -k*t

ln [A] / 0.220 M = - 4.0*10^-3 s^-1*230 s

ln [A] / 0.220 M = -0.92

now taking antiln from both side

[A] / 0.220 M = 0.398

So, [A] = 0.220 M * 0.398

= 0.0877 M

= 87.7 mM

So the concentration after 230 s is 0.0877 M or 87.7 mM

queen_honey_blossom answered 2 years ago

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