Question

For a reaction, $A+2B⟶C$, rate is give by $+\frac{d\left[C\right]}{dt}=k\left[A\right]\left[B\right]$, hence, the order of the reaction is:

• A. 3
• B. 2
• C. 1
• D. 0

Answer 1

The correct option is B 2

Rate $\left(\frac{+dC}{dt}\right)=k\left[A\right]\left[B\right]$
Thus, the order of reaction with respect to $A=1$
The order of reaction with respect to $B=1$
Total order of reaction $=1+1=2$