Consider the two rate laws:

(I) Rate = k [A]^1/2 [B]^3/2

(II) Rate = k [A]^3/2 [B]^–1

The correct statement among the following is-

In the reaction: \(\small {\mathrm{A}+2 \mathrm{~B} \rightarrow 6 \mathrm{C}+2 \mathrm{D},}\) if the initial rate \(-\dfrac{d[A]}{d t}\) at \(t=0\) is \(2.6 \times 10^{-2} \mathrm{M} \mathrm{~sec}^{-1},\) what will be the value of \(-\dfrac{d[B]}{d t} \text { at } t=0 \)?

In a reaction, the rate expression is, rate = K[A][B]^2/3[C]⁰, the order of the reaction is:

1. 1

2. 2

3. 5/3

4. zero

The reaction 2A + B + C $\to$ D + E is found to be a first-order reaction with respect to A, second-order reaction with respect to B, and zero-order reaction with respect to C. If the concentrations of A, B, and C are doubled, the rate of the reaction will be:

1. 72 times

2. 8 times

3. 24 times

4. 36 times

What is the rate equation for reaction 2A+ B $\stackrel{}{\to }$ C if the order of the reaction is zero ?

1.$<mspace\; width="1em"></mspace>k<mspace\; width="1em"></mspace>{\left[A\right]}^{0<mspace\; width="1em"></mspace>}{\left[B\right]}^0$

2. $k<mspace\; width="1em"></mspace>{\left[A\right]}^1{\left[B\right]}^0$

3. $k<mspace\; width="1em"></mspace>{\left[A\right]}^1{\left[B\right]}^1$

4. None of these

A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will: 

1. Remain unchanged 

2. Triple 

3. Increases by a factor of 4 

4. Double 

If the rate of the reaction is equal to the rate constant, the order of the reaction is: