The formula to calculate the rate of a reaction is:
\[ v = k [A]^x [B]^y \]
where \( v \) is the rate of reaction, \( [A] \) is the concentration of species A, \( [B] \) is the concentration of species B, \( x \) is the order of reaction with respect to A, \( y \) is the order of reaction with respect to B, and \( k \) is the rate constant.
A rate of reaction is defined as the change in concentration over time of two or more reactants. It can also be considered the change in concentration of the chemical product of the reaction over time.
Let's assume we have the following values:
Step 1: Raise the concentration of A to the power of x:
\[ [A]^x = 0.5^1 = 0.5 \]
Step 2: Raise the concentration of B to the power of y:
\[ [B]^y = 0.3^2 = 0.09 \]
Step 3: Multiply the results by the rate constant k:
\[ v = 0.1 \times 0.5 \times 0.09 = 0.0045 \text{ M/s} \]
Therefore, the rate of reaction is \( v = 0.0045 \text{ M/s} \).
