kinetics at times square final

kinetics at times square final - Sadaf Ayaz Precipitating...

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Sadaf Ayaz Precipitating in Central Park Professor Edmund Tam Lab Partners: Natalia and Gaby 04/07/2016 Sadaf Ayaz
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Professor Edmund Tam Lab Partners: Natalia and Gaby 04/07/2016 Kinetics at Times Square PART ONE: Description of Substances: Mossy Zinc Solid gray/blue circular pieces of zinc Magnesium ribbon Metallic silver/gray solid strips 2 M HCl Clear liquid Description of Zinc and Mg reaction with HCl: The Magnesium ribbon immediately reacted much faster than the Mossy zinc when placed in a flask containing HCl. The Mossy Zinc reacted so slowly that for a moment we had thought that a reaction was not happening, however, when we looked closer, we noticed slight fizzing and bubbling while the Magnesium ribbon had completely dissolved in approximately 25.3 seconds. Dilution Data: HCl concentration Calculations Volume of HCl 2M (2.0M)(xmL)= (2M)(25ml) x= 25mL 25mL 1.5M (2.0M)(xmL)= (1.5M)(25mL) x= 18.75mL 18.75mL
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1.0M (2.0M)(xmL)= (1.0M)(25mL) x= 12.5mL 12.5mL 0.75M (2.0M)(xmL)= (0.75M)(25mL) x= 9.37mL 9.375mL 0.5M (2.0M)(xmL)= (0.5M)(25mL) x= 6.25mL 6.25mL Length and Mass of Mg: Length of Mg- 1.5cm Mass of Mg- (0.37)(1.5cm) = (30.1)(x) x= 0.018g Concentration and Time data AND Temperature: Concentration: (2.0M) Time: Temperature Before: Temperature After: Trial 1: 17.5 sec 23.6 o C 24.8 o C Trial 2: 13.35 sec 23.6 o C 25.6 o C Concentration: (1.5M) Time: Temperature Before: Temperature After: Trial 1: 41.15 sec 23.2 o C 24.3 o C Trial 2: 40.0 sec 22.8 o C 24.2 o C Concentration: (1.0M) Time: Temperature Before: Temperature After:
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Trial 1: 55.9 sec 22.9 o C 25.0 o C Trial 2: 67.0 sec 22.2 o C 24.2 o C Concentration: (0.75M) Time: Temperature Before: Temperature After: Trial 1: 123.25 sec 23.2 o C 25.3 o C Trial 2: 119.09 sec 22.7 o C 24.6 o C Concentration: (0.50M) Time: Temperature Before: Temperature After: Trial 1: 194.4 sec 22.5 o C 24.9 o C Trial 2: 215.04 sec 23.2 o C 25.5 o C Results Tables: Plot of concentration of HCl in M (x-axis) vs tine in sec. (y-axis):
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Calculate the rate of reaction of Mg (grams of Mg divided by time in seconds) at each concentration: Trial 1: Concentration: Rate of reaction: 2.0 M (0.018g)/(17.5) = 1.02x10 -3 1.5 M (0.018g)/(41.5) = 4.3x10 -4 1.0 M (0.018g)/(55.9) = 3.2x10 -4 0.75 M (0.018g)/(123.25) = 1.46x10 -4 0.5 M (0.018g)/(194.4) = 9.26x10 -5 Trial 2: Concentration: Rate of reaction: 2.0 M (0.018g)/(13.35) = 1.3x10 -3 1.5 M (0.018g)/(40.0) = 4.5x10 -4 1.0 M (0.018g)/(67.0) = 2.68x10 -4 0.75 M (0.018g)/(119.9) 1.50x10 -4 0.5 M (0.018g)/(215.04) 8.37x10 -5
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Plot of concentration of HCl in M (x-axis) vs. rate of reaction of Mg in g/sec (y-axis): Linear plot that involves concentration vs. rate: Trial 1: Trial 2:
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Focus Questions: 1. How does varying concentration affect the rate of a chemical reaction? There is a direct relationship. When you increase the concentration, the reactants increa the rate of reaction. 2. What is the rate law for the reaction between Magnesium and Hydrochloric acid? The rate law for the reaction between Magnesium and Hydrochloric acid is 3.5 x 10 -4 PART TWO: Description of Substances: 0.2M IO 3 - Colorless liquid 0.001 HSO 3 - Clear liquid Description of Reaction: After mixing the test tubes with IO 3 - and HSO 3 - three times, we knew that the reaction had completely taken place when it turned a blue color. We noticed that as the amount of water increased, the time it took for the reaction to take place and the color to change increased.
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