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Consider the reaction \mathrm{2 A+B \rightarrow Products}, which follows the rate low : \mathrm{R=K(A)^{2}(B)}. At on initial time,\mathrm{[A]=0.2 M\, \&\, [B]= 0.1 M }. After 20 seconds,\mathrm{[A] } decreases to \mathrm{0.1\, M}.what is the average rate of the reaction during this time interval?

 

Option: 1

0.001 \mathrm{M} / \mathrm{s}


Option: 2

0.002 \mathrm{M} / \mathrm{s}


Option: 3

0.005 \mathrm{M} / \mathrm{s}


Option: 4

0.004 \mathrm{M} / \mathrm{s}


Answers (1)

The average rate is given by the formula as follow:

\mathrm{\text { Average rate } =\frac{\Delta(A)}{\Delta t}=\left[\frac{A_{\text {final }}-A_{\text {Initial }}}{T_{2}-T_{1}}\right]}
                            \mathrm{=\frac{0.1-0.2}{20}=-0.005 \mathrm{~M/s}}

Since rate is a positive quantity, the magnitude of the average rate is \mathrm{0.005 \mathrm{M/s}}. Negative sign indicates that concentration of \mathrm{A} is decreasing with time.

 

Posted by

Ramraj Saini

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