How do you find the rate(mole rxn/L s) from .00014 M or Iodine, .57 M or acetone, and .18 M of H+ and 16.8 seconds?
To find the rate of a reaction in terms of moles per liter per second (mol rxn/L s), you'll need to use the stoichiometry of the reaction and the concentration of the reactants.
First, determine the balanced chemical equation for the reaction you're studying. Without knowing the specific reaction you're referring to, it's not possible to provide the exact equation. Let's assume a generic reaction equation:
aI2 + bCH3COCH3 + cH+ → d products
Next, identify the reactants and their respective coefficients in the balanced equation. In this case, the reactants are Iodine (I2), acetone (CH3COCH3), and H+.
In the generic equation, the coefficients for I2, acetone, and H+ are a, b, and c, respectively.
Given the concentrations of the reactants (0.00014 M or Iodine, 0.57 M or acetone, and 0.18 M of H+), you can substitute these values into the balanced chemical equation.
Using the given concentrations and the balanced equation, consider the following:
1. Divide each reactant's concentration by their respective coefficient in the balanced equation.
- For Iodine (I2): 0.00014 M / a
- For acetone (CH3COCH3): 0.57 M / b
- For H+: 0.18 M / c
2. Determine the smallest of these values. This will be the "rate" value.
Finally, since you also provided a time of 16.8 seconds, divide the rate value obtained above by the time (in seconds) to get the rate in mol rxn/L s.
Please note that without the specific reaction equation, it is not possible to provide the exact rate value.