A) unit of k must be\[{{s}^{-1}}\]
B) \[{{t}_{1/2}}\]is a constant
C) rate of formation of C is twice the rate of disappearance of A
D) value of k is independent of the initial concentrations of A and B
Correct Answer: C
Solution :
\[2A+B\xrightarrow{{}}C\] \[Rate=k[A][B]\] It represents second-order reaction. Thus unit of k is \[{{M}^{-1}}{{s}^{-1}}\] Therefore, option (a) is false. \[{{T}_{50}}\]is dependent of concentration but not constant. Therefore, option (b) is false. \[-\frac{1}{2}\frac{d[A]}{dt}=\frac{d[C]}{dt}\] thus option (c) is correct.
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