Determination of the order of a reaction lab report

In this experiment, crystal violet and NaOH form a complex that changes from transparent blue to colorless over time.

Reactions usually occur more rapidly when the reactants are in the gaseous state. Since this plot is also clearly non-linear, the reaction is not 2nd order.

Rate of Reaction of HCl & Mg Lab Answers

Activation energy is the minimum energy to start a chemical reaction. Rate laws are able to quantify the rate at which a reaction occurs; they are the basis of studying the kinetics of chemistry.

However, this was not the exact reaction that took place. The rate determining step, or slow step, must be step 1. Phase of The Reactants Reactions produce products by having the reacting molecules come into contact with one another.

We determined experimentally that the order for both H2O2 and I— was 1. Reactions do occur in pure liquids or in solid form but the rates tend to be rather slow because the reacting molecules are very restricted in their movement among one another, and therefore, do not come into contact as often.

Is the reaction 1st order? If the reaction is 2nd order, a plot of concentration versus time will result in a straight line. In conclusion, although there were some errors associated with this experiment, it was successful in determining the relationship between temperature and reaction rate.

One way to find the order is by first measuring the concentration of the products as time passes. Temperature of HCl vs. The reaction that occurred during this lab was the decomposition of hydrogen peroxide catalyzed with the presence of potassium iodide.

I then divided the initial rate laws for Parts I and II, which canceled out the hydrogen peroxide as the concentration of hydrogen peroxide did not change in these parts.

For example, in the hydrolysis of 2-chloromethylpropane: This mixture was mixed with a glass stirring rod for a few moments to ensure consistency. Since this plot is clearly linear, the reaction is 1st order.

Determining the Rate Law for the Crystal Violet-Hydroxide Ion Reaction

Once again, this can be avoided by performing the experiment in a closed room. Adding iodine, however, considerably speeds up the reaction. The cuvet again cleaned with a Kimwipe and was inserted into the spectrophotometer. The cuvet was then rinsed with the mixture two or three times and was then filled with the mixture.

The biggest diversion from this value was Part II, which was 2. The rate constant depends on the temperature of the reaction as higher temperatures would cause the rate to go up without any bearing on the concentration of the reactantsso we could not compare the rate constants of Parts IV and V, as they are at higher temperatures.

The cuvet was then inserted into the spectrophotometer and the spectrophotometer was zeroed. The rate is dependent on the concentrations and the orders of the reactants.

Lab Report: Reaction Order and Rate Laws

In the end, the order of both reactants was found to be 1. For example, if the order of the above reaction for A was 2 and the order for B was 1, the reactant A would affect the rate more than the reactant B.

We added KI to the hydrogen peroxide because KI is a known catalyst and it would speed up the reaction. This lab was somewhat free of error, with our rate constant values being relatively constant.

The exponential equation can be converted to the linear form by taking the logarithm of both sides: Catalysts are defined by being substances that increase or decrease the rate of a chemical reaction without being consumed in the process. Catalysts are incredibly useful and sometimes vital in chemistry because they are able to significantly change the rate of the reaction without interacting with the reaction itself.

Decomposition of Hydrogen Peroxide Lab Answers

Is the reaction 0th order? This may have caused a change in the pressure readings, which would have changed all of our results significantly.Graph 1 shows the relationship between change in temperature and the rate of reaction.

The trend shows that the as the temperature of the HCl increases, so does the rate of reaction. This is a polynomial relationship, which implies that the rate of reaction increases exponentially in relation to the increase in temperature. correct units. What happens to the reaction rate as the reaction proceeds?

Why? Determine the reaction order of OH. You will not likely obtain an integer value for the reaction order of OH. Report the reaction order to two decimal places. There are resources on the web that may guide you. POSTLAB ACTIVITY You will be turning in. Objective: To study the effect of reactant concentration on the rate of the reaction between sodium thiosulfate and hydrochloric acid and to determine the order of each reactant and the rate law for the reaction.

2 HCI(aq) +. The order of the reaction with respect to H₂O₂ can be studied conveniently by choosing condition such that there is practically constant excess of HI. The kinetics then follow the first order. The reaction that occurred during this lab was the decomposition of hydrogen peroxide catalyzed with the presence of potassium iodide.

The decomposition of hydrogen peroxide by itself is 2H 2 O 2(aq) -> 2H 2 O (l) + O 2(g). Introduction. The kinetics of a chemical equation is determined by its rate. The rate is the speed at which the reactants form into products. The rate is dependent on the concentrations and the orders of the reactants.

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Determination of the order of a reaction lab report
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