3. Carefully put an egg in a glass half filled with vinegar. Replace the vinegar on the second day. Place the covered glass with the vinegar and egg in a safe place for one week without disturbing it. After one week, pass a light through the egg using a flashlight. N.B. DO NOT BOIL AND EAT THE EGG. A. Results and observation. Equation: HC2H3O2 + CaCO3 calcium acetate + H20 + carbon dioxide B. Calculation: If 9.02 x 1024 particles of vinegar (HC2H3O2)HC2H3O2) is added to 16.5 moles of eggshell (CaCO3) and 6.35 moles g of calcium acetate is formed. What are the (a) theoretical yield, (b) actual yield and (c) percent yield

3. Carefully put an egg in a glass half filled with vinegar. Replace the vinegar on the second day. Place the covered glass with the vinegar and egg in a safe place for one week without disturbing it. After one week, pass a light through the egg using a flashlight. N.B. DO NOT BOIL AND EAT THE EGG. A. Results and observation. Equation: HC2H3O2 + CaCO3 calcium acetate + H20 + carbon dioxide B. Calculation: If 9.02 x 1024 particles of vinegar (HC2H3O2)HC2H3O2) is added to 16.5 moles of eggshell (CaCO3) and 6.35 moles g of calcium acetate is formed. What are the (a) theoretical yield, (b) actual yield and (c) percent yield

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The energy can be used with hydroelectric power plants to save energy. a. Fuel O b. Wind O c. Geothermal d. Biomass are formed by the decomposition of dead animals and plants under the earth for a long time O a. Ethane Gas O b. Uranium c. Fossil fuels O d. Biomass
How will you prepare 70 mL of 0.8% (w/v) CsCl? A. Put 0.56 g CsCl into a beaker then add 64.4 mL distilled water. B. Put 0.056 g CsCl into a beaker then add distilled water until it reaches the 70 mL mark. C. Add 5.6 g CsCl to 70 mL distilled water into a beaker. D. Add 0.56 g CsCl into a beaker then add 70 mL distilled water.
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A ring with a mass of 14.8g is tossed into a fire and then removed. The ring’s temperature went from 23.2oC to 55.8oC. During this process, the ring gained 214J of heat. Of what pure metal is the ring composed? A. copper B. iron C. gold D. aluminum
A hot cup of tea placed near an open window to cool. Which of the following statements best describes this situation? a. The tea is the surroundings and gains heat from the system. b. The tea is the surroundings and loses heat to the system. O c. The tea is the system and gains heat from the surroundings. d. The tea is the surroundings and neither gains nor loses heat. e. The tea is the system and loses heat to the surroundings.
Select from the list below, the Kavalue of aluminium nitrate, Al(NO3)3. (You will have to do a bit of research to answer this question.) A. 6.2 x 10-8 B. 1.8 x 10-5 C. 7.9 x 10-6 D. 7.5 x 10-3
Part C: energy in changes of state C1. Mass of empty calorimeter cup with lid C2.Mass of calorimeter with lid+water 6.835 g 107.15g 1 °C C3 Final water temperature Initial water temperature 22 °C C4 Mass of calorimeter with lid+water+melted ice 135.64 g Calculations C5 Mass of water C6 Temperature change C7 Calories lost by water °C cal cal Calories used to melt ice C8 Mass of ice that melted C9 Heat of fusion (calories to melt 1 g of ice) Show calculations for C7 Calories lost by water, C8 Mass of ice that melted and C9 heat of fusión
What are the requirements for a formation reaction? Select one or more: a. the formation of one mole of a compound b. the reactants are elements in their standard states c. the formation of a solid d. the reactants must all be in the gaseous state e. the ΔHf° must be equal to 0 f. the balancing coefficients for each reactant must be 1 g. the product must be in the gaseous state
9. Determine the amount of heat released when 5.0 g of ethane(C₂H6) are combusted. (AH comb. =-1423 kJ/mol) A. 284.6 kJ B. 236.5 kJ C. 7115 kJ D. 1423 kJ
Milk left outside at room temperature spoils faster than milk kept cold in the refrigerator. Explain this observation in terms of how temperature affects the speed of a chemical reaction.