For a reaction whose rate expression is : Rate $ = k{[A]^{1/2}}{[B]^{3/2}}$, the order would be
For a reaction whose rate expression is : Rate $ = k{[A]^{1/2}}{[B]^{3/2}}$, the order would be
- A
$1.5$
- B
$2$
- C
$3$
- D
$1$
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Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?
Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?