Question

For a reaction of the type $A+B\to$ products, it is observed that doubling the concentration of $A$ causes the reaction rate to be four times as great, but doubling the amount of $B$ does not affect the rate. The rate equation is?

• A. Rate$=K\left[A\right]\left[B\right]$
• B. Rate $=K{\left[A\right]}^2$
• C. Rate $=K{\left[A\right]}^2\left[B\right[$
• D. Rate $=K{\left[A\right]}^2{\left[B\right]}^2$

Answer 1

The correct option is B Rate $=K{\left[A\right]}^2$

Given:

Reaction $A+B\to Products$

On doubling the concentration of $A$ rate increase by $4times$

so rate w.r.t $A$ will be $2$

$Rate=[A{]}^2$

But on doubling the the concentration of $B$ Rate remain unchanged so

so rate w.r.t $B$ will be $0$

$Rate=[B{]}^0$

Hence total $Rate=\left[A{]}^2\right[B{]}^0$

Option B is correct