In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 10mL 4.0 M acetone + 10mL 1.0 M HCl + 10mL 0.0050 M I2 +20 mL H2O....On question #2. a.) I determined the: Rate = 4.0 *10^-6...... But part b.) question has me confused: Given the rate from part a, and the initial concentration of acetone, H+ ion, and I2 in the reaction mixture, write equation 3 [rate = k (acetone)^m(I2)^n(H+)^p] as it would apply to the mixture.....Help?

Question

In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 10mL  4.0 M acetone + 10mL  1.0 M HCl + 10mL 0.0050 M I2 +20 mL H2O....On question #2. a.) I determined the: Rate = 4.0 *10^-6...... But part b.) question has me confused: Given the rate from part a, and the initial concentration of acetone, H+ ion, and I2 in the reaction mixture, write equation 3 [rate = k (acetone)^m(I2)^n(H+)^p] as it would apply to the mixture.....Help?