Question

For the given reaction,
$2A+3B+C\to \text{products}$
Order of reaction with respect to A, B and C are 3, 1 and 0 respectively. What will be the rate law of the given reaction?

• A. $R=K\left[A{]}^2\right[B{]}^3\left[C\right]$
• B. $R=K\left[A{]}^2\right[B{]}^3$
• C. $R=K\left[A{]}^3\right[B{]}^1[C{]}^0$
• D. $R=\left[A\right]\left[B{]}^2\right[C{]}^3$

Answer 1

The correct option is C $R=K\left[A{]}^3\right[B{]}^1[C{]}^0$

Order of a reaction:
For a given reaction:
$aA+bB+cC\to \text{Products}$
If,
$\text{Rate}\propto \left[A{]}^p\right[B{]}^q[C{]}^r$
Overall order of the reaction is :
$(p+q+r)$
where,
p: order of reaction with respect to A
q: order of reaction with respect to B
r: order of reaction with respect to C

For,
$2A+3B+C\to \text{products}$

$\text{Order of reeaction with respect to A is 3}$
$\text{Order of reeaction with respect to B is 1}$
$\text{Order of reeaction with respect to C is 0}$

Hence, the rate law of the reaction is
$R=K\left[A{]}^3\right[B{]}^1[C{]}^0$
Also,
$\text{Order of reaction is}=4$