Determining the enthalpy change for the thermal decomposition of potassium hydrogen carbonate into potassium carbonate. Controlled Variables: 1. Volume of HCl ± 0.5 cm3 (± 2%) 2. Concentration of HCl‚ 3. Same mass of K2CO3 and KHCO3 within specified ranges of 2.5 – 3.0g and 3.25 – 3.75g respectively 4. Same calorimeter used i.e. polystyrene cup is used in this experiment 5. Same thermometer will be used ± 0.10K 6. Same source of K2CO3‚ KHCO3 and HCl Raw Data Results: The raw
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Copper Reactions Rodney Jay C. Ridao Florencio Louis Pascual Relao De La Salle University- Dasmariñas Dasmariñas Cavite Philippines ABSTRACT The Copper Reactions experiment was demonstrate by adding the reagents like 16M HNO3‚ Distilled water‚ 6M NaOH‚ 6M H2SO4‚ Acetone‚ Zinc metal and Methanol into the beaker with the copper wire. The experiment was also demonstrated to observe how copper reacts while different reagent were being added. It was also demonstrated to practice the common laboratory
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time in various ways such as sweating from climate changes or physical activities or maybe even from illnesses or various health problems. We loos water from the body by breathing processes‚ sweating and digestion so its very important we maintain hydration at all times‚ but remember we can also over hydrate and loss essential vitamins and minerals through urine‚ but by regulated water intake through drinking water or eating foods that contain water we can maintain
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The Enthalpy of Formation of Magnesium Carbonate By: Jessica Miller T.A: Thomas Lab Partner: Rebekah Melanson Thursday Lab Room 106 Chemistry 1001-A Due Date: Thursday February 3rd 2011 Abstract The purpose of this experiment was to determine the enthalpy of formation of magnesium carbonate in a lab setting. This was done using a calorimeter‚ which was calibrated by adding a known amount of both hot and cold water. Following the calibration of the calorimeter‚ HCl was placed into the empty calorimeter
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mass of copper wire was 1.250g but the recovered copper was only 0.120 subtracting the mass of the recovered copper with beaker from the tare beaker mass. So the percentage yield resulted only to 9.6% it is very little‚ and it may be due to many possible sources from doing the steps. Adding too much or too little of a compound to the copper solution‚or the loss of copper during transport or by being left on the stirring rod. Another situation which was a source of error is when the copper solution
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believed that the native peoples did not dare to approach the villagers because they feared the guns and dogs. Chapter Three: What gift did Jamie receive when the supply ship docked? When the supply ship docked‚ the gift Jamie received was a copper flute which he immediately began playing. Explain how the seal hunt illustrates Jamie’s feelings towards wildlife. The seal hunt illustrates Jamie’s feelings towards wildlife because when he saw the seal die‚ he was enraged immediately and spontaneously
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Determining an enthalpy change of a displacement reaction Aim: To determine the enthalpy change for the displacement reaction between zinc powder and copper (II) sulphate solution. Zn (s) + Cu2+ (aq) → Cu2+ (s) + Zn2+ (aq) Theory: For the displacement reaction‚ an excess amount of zinc powder is added to the measured amount of aqueous copper (II) sulphate. The temperature change over a period of time has to be measured and thus‚ the enthalpy change for the reaction can be measured. The equation
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Name Lab Partner Name(s) Thermodynamics‚ Enthalpy of Reaction Lab March 27‚ 2014 I. Purpose The purpose of this lab is to learn how to determine the heat of reaction. II. Safety 1. Wear appropriate safety attire (goggles‚ aprons‚ hair tie‚ etc.). 2. Do not directly inhale or ingest chemicals. 3. Understand safety information regarding the chemicals being handled during the lab (hydrochloric acid‚ sodium hydroxide). 4. Be aware of how to operate all lab equipment. 5. Clean hands
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destroys its lattice structure and the individual cations and anions dissociate through the body of the water. This ionic dissociation results in the surrounding water molecules getting attracted to the released ions (Lewis & Evans‚ 2011) and forming hydration shells. This process is referred to as dissolution (Lower‚ 2013). Sometimes‚ the dissolved ions may collide with each other and recrystallize (Silberberg‚ 2010). According to Reed (2013)‚ if enough salt is added to the water then a saturated solution
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EXTRACTION OF COPPER FROM OXIDISED COPPER ORE Aim: To analyse how copper is obtained from oxidised copper ore using the processes of leaching‚ solid-liquid separation‚ displacing and electrowinning. Method: Refer to ‘Extraction of Copper from oxidised Copper Ore’ document pages 1-2 Results: Leaching: The blue particles in the copper ore which is copper was dissolved in the sulphuric acid and the solution turned into a blue colour. There was also sediment that was floating around
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