Observing a Limiting Reactant An experiment was carried out to predict the limiting reactant in a chemical reaction between Magnesium and Hydrochloric acid‚ using the mole concept. Limiting Reactant: It is the reactant that will deplete or will be used up first during a chemical reaction. Limiting reactant also determine how long the reaction will last for. Balanced Equation: Mg + 2HCl = MgCl2 + H2 The balanced equation is needed to determine the mole ratio between the two reactants. From
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Restoring Balance LeChâtelier’s Principle and Equilibrium Introduction Chemical equilibrium is a true balancing act. What happens when the balance is disturbed? The purpose of this lab is to observe the effects of concentration and temperature on equilibrium and to visualize how balance can be restored based on LeChâtelier’s Principle. Background Not all chemical reactions proceed to completion‚ that is‚ to give 100% yield of products. In fact‚ most chemical reactions are reversible
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start our experiment‚ then‚ using a pipet‚ added 3 ml of water to test tube 1‚ and 3 ml of sucrase stock solution to test tubes 2‚ 3‚ and 4. We left test tubes 1 and 2 untreated‚ while we treated test tube 3 with 10 drops of concentrated HCl (hydrochloric acid) and test tube 4 with 10 drops of concentrated NH4OH (ammonium hydroxide). We then added with a pipet 2 ml of a 1% sucrase solution to each of the four test tubes. We mixed the contents of the test tubes by swirling them and allowed them to stand
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Thermochemistry Laboratory Report Abstract The purposes of these three experiments are to determine the heat capacity of a calorimeter and with that data‚ confirm Hess’s Law and observe enthalpy changes within reactions. By measuring the change in temperature that occurs with the interaction of two different reactants‚ we were able to determine both the calorimeter constant and the change in enthalpy of a given reaction. The results were rather mixed‚ as some numbers more closely resembled the
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water but insoluble in dichloromethane. Because aspirin is a reasonably strong acid‚ it can be converted to the salt‚ sodium acetylsalicylate‚ by reaction with the basic sodium hydroxide. While the two layers are thoroughly mixed‚ the aspirin will react with the sodium hydroxide in the bottom layer‚ which then migrates to the aqueous layer and can be easily separated in a separatory funnel. Adding some dilute hydrochloric acid to the aqueous solution restores free aspirin as an insoluble white solid;
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Christina A. Barazona September 15‚ 2014 ABSTRACT The effect of molecular weight on the rate of diffusion was figured by using a glass tube and an agar-water gel. In glass tube test‚ two cotton plugs submerse with two different substances – hydrochloric acid (HCL) and ammonium hydroxide (NH4OH) on the other end of the tube. By their molecular weight‚ NH4OH has a small molecular weight that diffuses at a faster rate. While the formation of a white cloud was first occurred at the end of the tube containing
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Chemical Proportionality (Carbonate and Hydrochloric Acid) Introduction: The purpose of this experiment is what happens when a solid substance‚ a metal carbonate is added slowly to a solution of an acid. We are finding methods of determining acid concentration. For us to balance certain equations‚ we will use a stoichiometry. For this experiment‚ we will need to set up the ratio and finding the concentration of HCI. Procedure: • Grab 4 different beakers. • Add a small amount of sodium carbonate
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present in cyclohexanol. This hydroxyl group can be removed by a process known as dehydration which results in the production of cyclohexene at the end of the dehydration process in the presence of a catalyst which‚ in this case‚ was 85% phosphoric acid. Dehydration can be defined as any chemical reaction which involves the removal of a water molecule from a substance. During the experiment‚ anhydrous calcium chloride was provided as a drying agent to ensure that pure cyclohexene was obtained‚ calcium
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w w ap eP m e tr .X w om .c s er UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education 0620/12 CHEMISTRY Paper 1 Multiple Choice May/June 2010 45 Minutes Additional Materials: *8778752636* Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended) READ THESE INSTRUCTIONS FIRST Write in soft pencil. Do not use staples‚ paper clips‚ highlighters‚ glue or correction
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Title Soda Ash: Great for the economy but detrimental to the body; So why is it involved in everyday life? Abstract Sodium carbonate‚ Na₂CO₃‚ commonly known as soda ash is used in the manufacturing of many economically important products such as the manufacturing of glass‚ chemicals‚ paper and detergents. Since sodium carbonate has a strong base‚ it is commonly used to neutralize acidic effects. Soda ash has a high pH in concentrated solutions and can irritate the eyes and skin as well
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