C what was the initial concentration of acetone

The rate constant for this first-order reaction is 0. How long in seconds would it take for the concentration of A to decrease from 0. The rate constant for the reaction is 0.

If the initial concentration of A is 0. After What is the half-life of this reaction assuming first-order kinetics? You have 0 free answers left. Get unlimited access to 3. Already have an account? Log in. Keith Leannon Lv2. Unlock all answers Get 1 free homework help answer. Ask a question. Join us on Discord. Principles of Chemistry Molecular Approach 3rd Edition, At room temperature, the half life of the reactant is min.

What is the constant of the decomposition reaction? Post Lab Questions: Answer question on this sheet. In this experiment we will first determine the rate law for a reaction by changing some of the above variables and measuring the rate of the reaction. During Part Two, we will explore the relation between the rate constant and temperature to discover the activation energy for this reaction.

Although orders of reaction can be any value, for this lab we will be looking only for integer values for the orders of reaction 0, 1, 2 are acceptable but not 0. As the acetone is iodinated and the iodine converted to the iodide anion, this color will disappear, allowing the rate of the reaction to be easily monitored.

Once the orders of reaction are known, we will be able to calculate the rate constant, k. In Part One of this experiment you will determine the rates of reactions, the orders of the reactants, and finally the rate constant at room temperature.

Procedure: Finding the rate, orders of reaction and rate constant, k at room temperature For each experiment listed below: measure out the appropriate quantities of 1.

Making sure not to spill any on your hands or clothes, measure out the appropriate amount of 0. Start the stopwatch as you add the iodine to the mL flask. Swirl the flask which helps to prevent acetone evaporation until the yellow color disappears, then halt the stopwatch. It may help to place the flask on a white piece of paper to help discern when the color disappears.

Record the time elapsed in seconds. Repeat this reaction mixture until two trials of the same experiment are within 20 seconds of each other. Determine the average time elapsed in seconds for this experiment. Repeat this process for each of the four experiments listed in the table below. Determine the concentration of each reactant acetone, HCl and iodine in each reaction mixture.

Example: Determine the concentration of iodine in experiment 1. Solution: Since M1 and V2 are the same as in the previous example, we see that only V1 has changed to Average each pair of times for each experiment then calculate the rate of the reaction.

Example: Experiment 1 required an average of seconds to go to completion. Experiment 2 required an average of seconds to go to completion. Find the rate of reaction for both experiment 1 and experiment 2. Next determine the order of the reaction with respect to each reactant m, n, and p. Show your work clearly in your lab report as to how you solved for m, n and p.

Example: Find the order of reaction with respect to iodine p using the information calculated above. Solution: Notice how in experiment 2 we doubled the concentration of [I2] while leaving the other reactants' concentrations HCl, acetone unchanged.

An effect upon the rate of the reaction will reflect the influence of the iodine only, and this will allow us to determine p. In these sample calculations, doubling the concentration of iodine to 0. Calculate k for each experiment. Example: Find the value of k for experiment 1 using the values supplied above and assuming that the order with respect to acetone m is one and the order with respect to HCl n is one. Solution: Using the information in experiment 1, the diluted concentration of acetone is 0.

In a reaction involving the iodination of acetone, the following reaction mixture was used: 5. What was the molarity of the acetone in the reaction mixture?