Whenever two chemicals react, the reacting molecules or ions must collide in order for the reaction to take place. If the reactants are forced to collide more frequently then the reaction should be faster. Two factors which can influence the frequency of collision are temperature and concentration. Increasing the temperature of the reactants causes them to move faster and thus collide more frequently. If the concentration of a reactant is increased, then there are more opportunities for collisions and so the reaction rate increases.
The purpose of this experiment is to measure the effect of temperature and concentration on the rate of a reaction, the formation of carbon dioxide from an Alka-Seltzer (or similar) tablet plopped into water. Alka-Seltzer tablets contain aspirin, sodium bicarbonate (NaHCO3) and citric acid. Carbonate (e.g., Na2CO3) and bicarbonate compounds react with acids to form carbon dioxide.
HCO3-1 + H+ ------------> H2O(l) + CO2(g)
and CO3-2 + 2 H+ -----------> H2O(l) + CO2(g)
In an Alka-Seltzer tablet the bicarbonate and acid are solids and so the H+ and CO3-2 ions are not free to move, collide and react. When plopped into water, the citric acid and sodium bicarbonate dissolve , freeing the ions to react. This results in the formation of the carbon dioxide gas and water as the reaction products. By measuring how fast the carbon dioxide is formed, we are measuring the rate of the reaction.
Stockroom: Things to borrow and return on the same day. You may work with one other person today.
Procedure:
The volume of CO2 formed is
directly proportional to the mass of CO2 formed and the mass of
NaHCO3 decomposed. The volume of the CO2 formed at 10
second time intervals is measured using the apparatus shown below.
Half-fill a copper bath with room temperature tap water. Measure and record the temperature of the water. Fill the larger Erlenmeyer flask with water and half fill the graduated cylinder with water. Attach the stopper to the large flask as shown above, leaving the smaller flask's stopper free. Place the other hose into the graduated cylinder so that the opening remains below the surface of the water.
Using a pipet bulb, blow air into the free stopper tube to force water from the large Erlenmeyer flask into the graduated cylinder to create a siphon. There should be no air in the hose that goes from the large flask to the graduated cylinder. If a siphon is successfully established, the water level inside the large flask can be raised or lowered by moving the graduated cylinder above or below the level of the flask. Check to be sure your set-up is siphoning.
Allow enough water to siphon into the large flask to essentially fill it, then pinch the water filled tubing with a pinch clamp to prevent the water from siphoning over. Empty the water in the graduated cylinder and reposition the hose into it.
Carefully place a vial of water taken from the water bath and an Alka-Seltzer tablet into the dry 250 ml flask (smaller flask). Put the stopper tightly into the flask, and remove the pinch clamp from the hose. A small amount of water will drain into the cylinder but should not siphon from the flask. (If it does, there is a leak that must be fixed). Hold the 250 ml flask in the water bath and swirl to start the reaction. Holding the cylinder below the bench level, record the volume of water displaced every 10 seconds until it is unchanged for 20 seconds. The most accurate results are obtained by marking the level of the water in the cylinder directly on the cylinder (use masking tape!) every 10 seconds. When gas evolution is over, read and record the volume measurements in your notebook using the markings on the cylinder.
Effect of temperature: Repeat the experiment using the same temperature. Also do two trials each for a high temperature reaction using hot water (from the facet) in the water bath and reaction vial. Be certain to measure and record your reaction temperatures.
Effect of concentration of reactants: How does the rate of the reaction and total volume of CO2 evolved depend on the size of tablet? Test this by cutting a tablet in half and measuring the rate of the reaction at room temperature with each half tablet. Be certain the tablets have the same approximate size and are in one piece. Do two trials with half a tablet, then do two trials with a whole tablet that has been broken into two pieces (2 "1/2" tablets). This will assure that you have the same surface area to mass of tablet ratio in all of the trials. Do all of these trials with half tablets at the same temperature of water in the water bath and in the reaction vial.
Effect of surface area: Compare the rate of 2 "1/2" tablets with the rate of one tablet. Which experiment has more surface area? Which one has a faster rate?
The tables of times and volumes along with the identification of reaction conditions will be in your results section. Use Excel to make plots of volume vs time. Use only the first 4 time points. Be certain to title each graph and label the axes. Several trials can be plotted on one graph . Normally a straight line can be drawn from the graph origin (0 sec, 0 mL) through the initial points in each trial. The slope of this line is a measure of the rate of evolution of CO2. It is expressed in units of ml CO2 per second. To find the slope (reaction rate), put the mouse over a data point and right click on it. Then, select "insert trend line", in the "trend-line" box, go to options and select "show equation on graph". If you did not empty out your graduated cylinder before each trial, you will need to set the "line goes through y axis" to whatever volume you had at time=0 sec.
Your data should be arranged in a neat table:
Summary of Trial Runs
| Temperature | Rate (slope) | Average Rate (Runs 1 & 2) | ||
|---|---|---|---|---|
| High Temperature (whole tablet) |
Run 1 | |||
| Run 2 | ||||
| Whole tablet (room temp) | Run 1 | |||
| Run 2 | ||||
| Half tablet (room temp) | Run 1 | |||
| Run 2 | ||||
| 2 Half tablets (room temp) | Run 1 | |||
| Run 2 |
For your conclusion restate the average rates of the reaction at each of the four experiments: using two temperatures for a whole tablet, using two half tablets and using a half tablet.
Compare the "two half tablets" with the "half tablet" to determine the effect of concentration. Compare the "two half tablets" with the "whole tablet" at room temperature to determine the effect of surface area. Which experiment provided more surface area?
Compare the whole tablet at room and high temperature to determine the effect of temperature.
Does the final amount of carbon dioxide that is produced (look at your values for CO2 at the very last time point) change with either temperature, concentration or surface area? Explain your results.
What are the possible sources of error in this experimental procedure? Remember to use complete sentences in well organized paragraphs.
Back to Biochemistry for Nurses at CSU, Stanislaus
Last edited by K. Stone on 03/13/08