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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, …show more content…
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
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.
I Know my reactants in this chemical reaction are Potassium Nitrate (KNO3) and Sugar (C12H22O11). According to "What Product Will Get When Sucrose and Potassium Nitrate Mix Burn?" Inorganic Chemistry .N.p.,n.d. Web.28Jan.2016. . "You will get Potassium carbonate (K2CO3), Carbon dioxide (CO2), Water (H2O) & Nitrogen gas (N2) as per the following reaction." This helps us understand that our rocket is a complete combustion chemical reaction because its products contains water and carbon dioxide. This can also let me balance out the equation for myself. 44 KNO3 + 5 C11H22O11 22 K2CO3 + 33 CO2 + 55 H2O + 22 N2 . Is the answer I got. This is how I got
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
I have been a snob. It is quite soft, but solid. It reacts with hydrochloric acid. like this 2 CaCO3 + 2 HCl â’ CO2 + CaCl2 + H2O. producing carbon dioxide, which is what we measured in the experiment. There are different factors affecting the rate of this reaction, such.
First, the volatile gases break apart and the atoms recombine with the oxygen to form water and carbon dioxide. This is called burning. The reaction for this is:
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).
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.
Hypothesis: It is predicted that when there is a higher amount of baking soda the rate of reaction will decrease as more baking soda is added each trial. This is predicted because when baking soda and vinegar react, they exchange atoms. In this case,they are exchanging a proton,which is a subatomic particle that makes atoms. In this reaction, baking soda will act as a base,and takes a proton from vinegar, which is an acid.The reaction releases gas because when the baking soda receives the proton, it transforms into water and carbon dioxide. When higher amounts of baking soda are added,it will be able to make an impact of the results by increasing the amount of gas produced.
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
The indicator solution made this occur. It caused the bag to puff up because it has high acidity levels and when mixed with the baking soda. This reaction was a exothermic reaction because heat was given off of the experiment. The catalyst or what caused the reaction to start was the indicator solution. This is because once the indicator solution was tipped over the reaction
MATERIALS AND METHODS Materials to be used will be 125-mL Erlenmeyer flask, 400-mL beaker, iron stand, iron ring, clamp, crucible tongs, 100-mL graduated cylinder, thermometer, aluminum foil, heating stove and burner (if possible). Reagent needed for the experiment was the unknown liquid
Obtain as close to .5g of copper wire, and record the mass to the closest mg. Make sure the wire is bent so it will lay as flat as possible in the bottom of a 250mL beaker. Then go to ¡§the hood¡¨ and add 4mL of 16M HNO3. Swirl the HNO3 around in the beaker with the copper until it has completely dissolved and you are left with a green/blue liquid. Then add 30mL of 3M NaOH and heat the solution on a ring stand with a Bunsen burner. The blue/green jelly will turn in to sort of a black dirt at the bottom of the beaker, make sure to stop boiling when the jelly turns black. Decant all excess liquid in the beaker. Do not remove any black precipitate. Add approximately 200mL of hot deionized water to the black precipitate. Decant all excess liquid again. Add 15mL of 6M H2SO4 and then under ¡§the hood¡¨ add 2g of Zinc metal to the solution. Once the Hydrogen has stopped bubbling add 10mL of HCl. Decant all excess liquid and transfer Copper metal to a glass dish and wash with deionized water. Rewash Copper metal with 5mL of Methanol. Decant and dry Copper metal on a hot plate, weigh and record results to nearest mg.
In this experiment I will use boiling tube, measuring cylinder, timer, hydrochloric acid(0.5 , 1.0, 1.5, 2.0, 2.5, 3.0 Moles), magnesium, test tube rack, clamp stand, a ruler and i will have to wear goggles to protect my eyes.
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
This can be checked by using a thermometer with each substance. Method: Tape a ruler to a wall at eye level. Make sure all substances being used ar at room temperature (37℃) with a thermometre Measure out 1 ml of the Hydrogen Peroxide (H2O2) solution with a plastic pipette, then transfer to a clean boiling tube. Repeat this another two times into two other boiling tubes.