Question

The velocity of a gaseous reaction is halved, whereas the volume of the pot is doubled. Calculate the order of reaction.

Hint:

The order of reaction can be determined using the rate equation: \( R \propto [C]^n \). Compare rate changes with concentration changes.

Answer 1

Step 1: The rate of reaction is given by: \[ \text{Rate} \propto [C]^n \] where \( n \) is the order of the reaction. Step 2: Since the volume is doubled, the concentration is halved: \[ [C]_{\text{new}} = \frac{[C]}{2} \] Step 3: The rate is also halved: \[ \frac{\text{Rate}_{\text{new}}}{\text{Rate}} = \left(\frac{1}{2}\right)^n = \frac{1}{2} \] Step 4: Comparing, \[ \left(\frac{1}{2}\right)^n = \frac{1}{2} \] \[ n = 1 \] Thus, the order of reaction is **1**.