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Effect of reaction rate on temperature
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The Examination of Chemical Reactions in Multiple Chemical Compounds to Identify Types of Energy Changes and Types of Reactions
The purpose of this lab is to investigate chemical reactions that takes place between different chemical compounds. The products formed through these reactions will be observed for physical properties and chemical changes.
Pour 100 mL of citric acid into an Erlenmeyer flask.
Fill a clay crucible with baking soda.
Measure and record the temperature of the citric acid solution.
Add baking soda into Erlenmeyer flask until the reaction stops.
Measure and record the temperature of the citric acid and baking soda solution, transferring no liquid.
Fill half a test tube with limewater.
Pour off the gas at the surface of the Erlenmeyer flask into the test tube half filled with limewater.
Stopper and shake the test tube.
Experiment B:
Pour hydrogen peroxide until the test tube is 1/3 full.
Measure the temperature of the solution.
Add a small amount of manganese IV oxide to the solution, and stopper the test tube.
Perform a gas test with a splint.
Measure the temperature of the solution. There are several safety procedures that were taken throughout the performance of this lab. Firstly,
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The sodium bicarbonate separates and reacts with the citric acid. The result product of this is carbonic acid (H2CO3 (aq)). However, carbonic acid by itself is not stable, so it decomposes into water, carbon dioxide, and sodium citrate. This results in bubbles of CO2 being formed. The reaction is endothermic because it absorbs heat and energy (does not occur spontaneously). The bond energies of the products are less than the bond energies of the reactants, thus, more energy is required to break the bonds in the reactants, rather than energy that is released when the product is formed. As a result, the temperature
5.) One at a time, place your test tubes in the water bath and heat the first test tube to 25 , the second to 50 , the third to 75, and the last to 100 degrees c. Remeber to stir with your stirring rod every so often.
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
Investigation of the reaction between hydrochloric acid and marble chips A chemical reaction is when two or more substance called reactants are chemically bonded to form a new product, as a result of the process, for a reaction to take place, the particles must have enough kinetic energy to collide and form new bonds , this is called a successful collision. The minimum amount of energy needed for a successful collision is activation energy, which is “The energy that an atomic system must acquire before a process can occur”. Chemical reaction is different to a physical reaction, chemical reaction are not reversible and results in a new product, however a physical reaction can be easily reversed as it only changed its state. The activation energy is able to loosen particles and enable them to from new bonds to produce new products. The faster the molecules are moving the bigger the chance of a successful collision, so the faster and stronger the reaction will be , the more kinetic energy a reactant has the easier it is for the new bonds the collide and produce new bonds.
Unit 7: Chemical Reactions: Students will understand the basic concepts of reactions, bonding, the “mole” and how this relates to the law of conversion of matter.
anyway) Note these factors affect the rate of the reaction, but not the final. amount of carbon dioxide produced). Why these factors affect it: higher temperature makes atoms move more. so they are more likely to bump into each other and react.
Second, a small sample of solutions must be collected and transferred to the beakers by pouring or pipetting from the 500 mL Erlenmeyer flasks containing the solution. Third, a clean wooden stick must be dipped into the solution, soaked for three to five seconds, and put to the flame created by the bunsen burner. It is very important to make sure that that the wooden stick should not catch fire and this may have to be done this several times in order to get a good color. Next, the color of the flame must be recorded in detail and the wooden stick must be ran under some running water to cool it off. Finally, the stick must be discarded into the trash and a new wooden stick must be obtained. Dipping the wooden stick into the solution and put toward the flame must be repeated for the remaining solutions and when you are all done all of the solutions , these solutions should be poured down the drain with a lot of water and rinsed with soap and water. Finally, the labels should be cleaned off, and the beakers should be left upside down to
Experiment to Compare the Enthalpy Changes of Combustion of Different Alcohols Introduction: This plan will try to outline how the experiment of comparing changes of combustion of different alcohols will be conducted and what results are expected. Background When chemical reactions take place they are often accompanied by energy changes. Chemical reactions most frequently occur in open vessels. That is, they take place at constant pressure. Enthalpy refers to energy at constant pressure (volume may vary).
Then, placing the thermocouple in the test tube to monitor the temperature by the labQuest. After a couple of readings of the solution in the hot bath, the test tube with the thermocouple inside it, should be transferred to the ice bath to monitor the temperature for a fixed length of time while the reading still running. This method should have been performed for all the trails with no additives for the trail
The output of both of these reactions is heat and light. The chemical reactions produce heat which causes the carbon atoms to rise. As they rise, they emit light. This is called incandescence. This is the same thing that causes a lightbulb to light up. It is the flame of the
Clean and dry all test tubes. 2. Set water bath 40oC temperature. 3. Level test tubes with the number 2,4,6,7,8, and10 for initials identification.
5. Measure 0 grams of baking soda on a scale pour onto the cork (Control test)
Tweezers Petri dishes Graduated Cylinders Test tubes Procedure: In 100 mL of water, put 3.5 grams of NaCl In a separate test tube, put 9 mL of the solution and 1 mL of water In another test tube, place 8
Add to each three boiling tubes 1 ml of the pH buffer solution being used first (hydrochloric acid or sodium hydroxide) with the pipette for, and pour into a boiling tube with the Hydrogen Peroxide solution. Use a pipelette to gather some of the mixture out of the three boiling tubes and place one drop from each boiling tube into three separate tile spotters. Use one drop of universal indicator on each solution in the tiles spotters to determine the correct pH that is needed for the first reaction (either 2,4,7,9,12). Add to each three boling tubes 1 ml of yeast, and start a timer as soon as the yeast is transferred to the boiling tubes. Time each boiling tube for 1 minute, then measure the O2 froth produced from the solution with a ruler at eye level.
Four of these include the release of energy, which occurred during the reaction, the substance got hot. Change is color, it turned into a yellowish white color after the reaction. There was a change is smell, it smelled like salt mixed with water. And lastly there was a change in state of matter. While the experiment was reacting it was in closed system, the experiment ended up puffing up.
In a 250ml beaker place 100mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved. After 1 minute measure the temperature and record it, do this for a further 2 minutes (3 minutes in total). Repeat this process for a total of 10 teaspoons.