Reaction Of The 0 1 M Hcl example essay topic

Experiment 34 Factors Affecting Reaction Rates Aim To observe the effects of temperature, catalysts, concentration, particle size and surface area on the rates of chemical reactions and to explain each of these effects in terms of kinetic-molecular theory. Equipment SS safety goggles SS 1 10 mL graduated cylinder SS 1 100 mL graduated cylinder SS 16 medium test tubes SS 1 test tube rack SS 2 250 mL beakers SS centigram scales SS 1 crucible tongs SS 1 thermometer SS 1 250 mL plastic bottle SS 1 ring stand SS 1 ring support SS 1 wire gauze SS 1 bunsen burner SS 1 dropper pipet SS 1 metal cutter SS stopwatch SS sticky tape Materials SS 0.1 M iron ( ) chloride, Feel 3 SS 0.1 M iron ( ) nitrate, Fe (NO 3) 3 SS 0.1 M sodium chloride, NaCl SS 0.1 M calcium chloride, CaCl 2 SS 0.1 M potassium nitrate, KNO 3 SS 0.1 M manganese chloride, M nCl 2 SS 3% hydrogen peroxide, H 2 O 2 SS 6 M hydrochloric acid, HCl SS 3 M hydrochloric acid, HCl SS 1 M hydrochloric acid, HCl SS hydrochloric acid, HCl SS zinc strips, Zn, 0.25 mm x 0.50 mm x 200 mm SS powdered zinc SS wood splints SS steel wool SS ice cubes SS aluminum foil SS paper towels SS distilled water Procedure Part A. Effect of Temperature on Reaction Rate The reaction of zinc metal with hydrochloric acid will be examined. 1. Pour 5.0 mL of 6 M hydrochloric acid into each of the three clean test tubes. Place one of the tubes in an ice water bath (ice-water mixture in 250 mL beaker). Place another in a hot water bath, maintained at 50 oC (heat the water in a 250 mL beaker over a bunsen burner).

Place the third tube in a test tube rack, at room temperature. Allow about 10 minutes for the tubes to reach the temperature of their surroundings. 2. Clean zinc strips with steel wool. Cut three small pieces of zinc to the same size; approximately 0.5 cm x 2.0 cm each. Save the remainder of the strip for later.

3. Drop one piece of zinc into each of the three test tubes containing hydrochloric acid. Cover each test tube loosely with a piece of aluminium foil and begin to time each of the reactions. Test for the identity of the gas produced by using tongs to hold a burning splint near the mouth of each of the tubes.

Note the duration of each reaction. Part B. Effect of a Catalyst on Reaction Rate The decomposition of hydrogen peroxide will be studied. 4. Measure 90 mL of distilled water into a clean 250 mL plastic bottle and add 10 mL of 3% hydrogen peroxide solution.

Label it as 0.3% hydrogen peroxide. This will be your test solution. 5. Rinse seven clean test tubes and a 10 mL graduated cylinder with the 0.3% hydrogen peroxide. Discard the rinses. Measure 5 mL of 0.3% hydrogen peroxide into each of the seven test tubes.

Place the test tubes in a rack. 6. Add 5 drops of each of the following solutions to separate test tubes of the hydrogen peroxide: 6 M hydrochloric acid, 0.1 M iron ( ) chloride, 0.1 M sodium chloride, iron ( ) nitrate, 0.1 M calcium chloride, potassium nitrate, 0.1 M manganese chloride. Flick each tube to mix its contents. Observe each solution and report the rate of gas evolution from each. Use the terms fast, slow, very slow or none to describe the rate of gas evolution.

Describe the catalytic activity as high, low or none. Record your observations. Part C. Effect of Concentration on Reaction Rate, at Constant Temperature The reactions of zinc metal with hydrochloric acid solutions of varying concentrations will be examined. 7. Pour 5 mL of each of the following hydrochloric acid solutions into separate clean test tubes: 0.1 M, 1 M, 3 M and 6 M. 8.

Cut four small pieces (1 cm x 1 cm) from the previously cleaned zinc strip. Again, save the remainder for later. Drop one piece of zinc into each of the acid solutions. Record the start time and the end time of each reaction. Part D. Effect of Particle Size or Surface Area on Reaction Rate The reaction of zinc metal with hydrochloric acid will be used to study the effect of particle size and surface area on the rate of reaction. 9.

Cut a piece of zinc (0.5 cm x 2.0 cm) from a clean strip of the metal. Determine the mass of the piece of zinc to the nearest 0.01 g and record. Place the piece of zinc in a clean dry test tube. 10.

Measure an equal quantity of powdered zinc into a clean second dry test tube. 11. Place both test tubes in a rack and add 5 mL of 1 M hydrochloric acid to each. Observe the reactions for several minutes and record your observations. 12. Follow your teacher's instructions for proper disposal of the materials.

Data Record Effect of Temperature on Reaction Rate Reaction Condition Reaction Duration (mins: secs) Burning Splint Test Result Ice Water 0^0 C 25: 39 High pitched popping sound Room Temp 24^0 C 5: 37 High pitched popping sound Hot Water 50^0 C 4: 00 High pitched popping sound Effect of Concentration on Reaction Rate Reaction Condition Reaction Duration (mins: secs) Observations 0.1 M HCl 20: 00 + Tiny bubbles emitted from the zinc metal. Very slow reaction. 1 M HCl 20: 00 + Small bubbles, more bubbly than 0.1 M HCl. Slow reaction.

3 M HCl 19: 48 Bubbly. 6 M HCl 5: 38 Bubbling largest bubbles. Very bubbly. Emitting a gas / smoke. Fastest Reaction.

General observation: reactions sped up and were more active, ie. more and bigger bubbles, as time passed and more zinc decomposed. Note: Due to time restrictions, the exact duration of the reactions is unsure, but continued past twenty minutes. Effect of Surface Area on Reaction Rate Substance Tested Observations Sheet Zinc Bubbling slightly, small bubbles emitted from zinc. Powdered Zinc Bubbling quite a bit. Zinc dissolving fast, turning into clumps. Liquid turns dark grey in colour.

The faster of the two reactions. Data Analysis 1. Write a balanced equation for the reaction between hydrochloric acid and zinc metal. 2 HCl (aq) + 2 Zn (s) 'a 2 Z nCl + H 2 (g) 2. Write a balanced chemical equation for the decomposition of hydrogen peroxide. H 202 (aq) 'a H 2 (g) + O 2 (g) 3.

Which ionic compounds used in Part B were effective catalysts? 4. Examine the data in table 34.2 and identify the ion responsible for the catalytic activity. 5. Many reaction rates approximately double for every 10^0 C increase in temperature. Are the results you obtained in Part A consistent with this general statement?

6. How does the surface area of a substance change as it is broken down into smaller pieces? When a solid substance is broken down into smaller pieces, it increases the surface area of the particles that is exposed to the other reactant particles. And with a greater surface area of particles exposed to reacting particles, comes an increase in the reaction rate. Conclusions 1.

Describe in your own words the effect of temperature on the rate of a reaction. Explain this effect in terms of the collision theory of reactions. In Part A of the experiment, we observed that the reaction in the hot water, 50 oC, occurred at a faster rate in comparison to the cold 0 oC water, where the reaction took over six times longer. To conclude, reactions occur faster at higher temperatures and slower at lower temperatures. Raising the temperature will speed up a reaction, whereas lowering the temperature will slow a reaction down.

At higher temperatures, the particles of the reactants move more and with a greater energy than at lower temperatures, causing more frequent collisions between them which causes a faster formation of products. Increasing the temperature increases the number of particles that have enough kinetic energy to react when they collide. At a higher temperature, more colliding molecules are sufficiently energetic to slip over the activation energy barrier to become products. 2. Describe in your own words the effect of concentration on the rate of a reaction. Explain this in terms of the collision theory of reactions.

We observed in Part C, that the reaction of zinc with the most concentrated solution, 6 M hydrochloric acid, occurred the fastest. The reaction of the second most concentrated solution, 3 M HCl, occurred the second fastest. After twenty minutes, the reactions with the zinc of the two other solutions of hydrochloric acid, that were not as concentrated [1 M and 0.1 M], had not yet finished. However, it can be predicted that, if more time was allowed, that the reaction of the 1 M HCl would have been completed before the reaction of the 0.1 M HCl. In conclusion, the more concentrated the reactants are, the faster the reaction will occur. In a more concentrated substance, there are more particles in the fixed volume.

This means that the collisions between the reactant particles will be more frequent and therefore the reaction occurs faster. Increasing the concentration of the reactants will increase the reaction rate. 3. Describe in your own words the effect of particle size or surface area on the rate of a reaction. The total surface area of a reactant is a contributing factor to the reaction rate.

The smaller the particles, the larger the surface area of those particles. An increase in the surface area of the particles increases the frequency of the collisions between the particles of the reactants because more of the reactant is exposed to the other. This was evident in Part D of the experiment [Effect of Particle Size or Surface Area on Reaction Rate]. When observing the reaction of zinc metal with hydrochloric acid, we noticed that as the solid zinc became dissolved, its particles broken down and separated, the reaction became more active and sped up. This was because the particles became smaller, which increases the particles's surface area, which in turn increases the rate of the reaction. 4.

Describe in your own words the effect of a catalyst on the rate of a reaction. A catalyst is a substance that increases the rate of a reaction without being used up itself in the reaction. Catalysts increase the rate of a reaction by lowering the activation energy barrier, that is, they allow a reaction to occur at a lower energy than is usually required. With a lower activation energy barrier, the reaction is initiated faster and therefore more reactants can form products within a given time..