Mole Ratio of Chemical Reactions Essay

accusatoryIn this experiment, you will determine the government issue of walls of reactants and products present in the reaction of cop and silver gray nitrate, and target their mole-to-mole ratio. The mole-to-mole ratio relating to the fade of hair and the formation of silver metal will be used to publish the quietusd comparison for the reaction. The reaction of shit metal with silver nitrate solution is a hit replacement reaction, represented by the quest unbalanced equation Cu(s) + AgNO3(aq) Cu(NO3)2(aq) + Ag(s) The values of the coefficients behind be refractory experimentally by measuring the tummy of copper outfit that reacts with the potful of silver that is produced in the preceding(prenominal) reaction.BACKGROUND MATERIALS NEEDEDThe reaction of copper and silver nitrate in aqueous solution provides an kindle display of chemistry in action delicate silver crystals begin to grow on the equip surface and the colour of copper(II) ions gradually appears in the solution. Stoichiometry is the area of chemistry that deals with the numerical relationships and mathematical proportions of reactants and products in a chemical reaction. One of the most important lessons of stoichiometry is that the amounts of reactants and products in a chemical reaction are link to one an other(a) on a mole basis. Chemical reactions are normally represented by balanced chemical equations. The coefficients in a balanced chemical equation summarize the relative number of moles of each reactant and product involved in a chemical reaction. The ratios of these coefficients represent the mole-to-mole (or simply mole) ratios that govern the disappearance of reactants and the appearance of products. Knowing the mole ratios in a balanced chemical equation is essential to work out stoichiometry problems.General Chemistry 1Lab Acetone Copper wire 3 M HNO3 AgNO3, silver nitrate 50 mL beaker 100 or 150 mL beaker Toothpick Stirring rod stifle bottle 50 mL measuring c ylinder SAFETY PRECAUTIONS Nitric acid is a sulfurous liquid and strong oxidizer. Silver nitrate is a corrosive square(p) and is toxic by economic consumption it will stain skin and clothes. Acetone is a flammable liquid avoid contact with flames and other sources of ignition. Avoid contact of all chemicals with eyes, skin, and clothing. Wash hands thoroughly with soap and peeing system before leave the laboratory area. Page 1 PROCEDURE 1. Obtain a clean, ironical 50 mL beaker. cautiously add 1.40 1.60 g of silver nitrate crystals to the beaker. Caution use a spatula to transfer the solid. Do non touch the silver nitrate and carefully clean up whatever spilled material on the balance or the bench top. 2. Measure and leger the exact peck of silver nitrate to the nearest 0.01 g. 3. suffer the beaker with 30 mL of distilled water and stir the mixture with a stirring rod until all the solid has dissolved. Rinse the stirring rod over the beaker with a little distilled water . 4. Take a piece of copper wire and loosely coil it. 5. Find the initial mass of the copper wire to the nearest 0.01 g and record it. 6. Use a toothpick to suspend the copper wire in the silver nitrate solution. The copper wire should not be touching the bottom or sides of the beaker. 7. Carefully add 3 drops of 3 M HNO3 to the beaker.Do NOT stir the solution. 8. Allow the beaker to sit on the lab bench for 15 minutes. Try not to jostle or shake the suspended copper wire in any way. 9. Observe the signs of chemical reaction occurring in the beaker and record all observations. 10. While the reaction is taking place, estimate a 100 or 150 mL beaker with your name and class session. Measure and record the mass of this beaker. 11. After 15 minutes, gently lift the toothpick to remove the copper wire from the solution. 12. Holding the wire with the woody toothpick, place the copper wire above the 100 or 150 mL beaker. Rinse the wire with a steady stream of distilled water from a wash bottle. The silver crystals should easily fall take the wire into the beaker. Gently shake the wire and rinse with General Chemistry 1 Lab water until no more silver adheres to the wire. notational system Use a total of about 40 mL of distilled water. 13. When all of the silver has been removed, lift the copper wire out of the beaker and place it in another beaker containing dimethyl ketone.The acetone will clean the wire surface and allow it to dry more quickly. Note Several groups can share this same rinse beaker of acetone. 14. Remove the copper wire from the acetone beaker and allow it to air dry for 3-4 minutes. 15. Measure and record the final mass of the copper wire. Note the appearance of the leftover wire and record your observations. 16. Examine the beaker containing the silver product. Most of the silver should have settled into a dense mass at the bottom of the beaker. Carefully decant the liquid into a waste flask to remove most of the water. Note Try not to lose any of the solid in the process. 17. Rinse the solid with 5-10 mL of distilled water from a wash bottle. Decant the rinse water into the waste water flask as well. 18. retell the rinsing and decanting cycle with a second portion of distilled water. 19. Discard the waste water in the bighearted beaker in the fume hood. 20. When all of the water has been decanted, place the labelled beaker containing the silver product on the thaw tray in the fume hood. 21. Allow the solid to dry overnight.22. When the solid is dry, measure and record the final mass of the beaker plus silver solid. Page 2 PRE-LAB QUESTIONS 1. Define a. Law of Conservation of Matter b. Molar mass c. Mole d. Stoichiometry e. Limiting reagent 2. Solve a. Using the balanced equation for the reaction of aluminum with iodine, answer the following questions 2 Al (s) + 3 I2 (s) Al2I6 (s) i. How galore(postnominal) moles of Al2I6 are produced by the reaction of 4.0 mol of aluminum? ii. How many moles of I2 are requisite to r eact exactly with 0.429 mol of aluminium? b. What mass of sodium hydroxide, NaOH, would be required to produce 16 g of the antacid milk of magnesia magnesium hydroxide, Mg(OH)2 by the reaction of magnesium chloride, MgCl2, with NaOH? MgCl2 (aq) + 2 NaOH (aq) Mg(OH)2 (s) + 2 NaCl (aq) i. Which reactant is limiting? ii. How much water will the reaction produce? POST-LAB QUESTIONS 1. Calculate the mass and moles of copper wire that reacted in this experiment. draw your calculations. 2. Calculate the mass and moles of the silver produced in this experiment. Show your calculations. 3. Determine the mole ratio the ratio of the number of moles of silver to the number of moles of copper. Round the result to the nearest whole number. Show your calculations. 4. Use the silver/copper mole ratio to write a balanced chemical equation for this reaction of copper and silver nitrate. 5. What was the limiting reagent in this experiment? Show all calculations and explain your answer. 6. preconditi on what you know about copper, silver nitrate and this kind of single replacement reaction, what would you have predicted the balanced chemical equation to be? 7. Explain the possible differences between Question 4 and Question 6. 8. Do the results of your experiment support the Law of Conservation of Matter? Explain. c. Calculate the mass of oxygen gas, O2, required for the combustion of 702 g of octane, C8H18. 2 C8H18 + 25 O2 (g) 16 CO2 (g) + 18 H2O (l) d. A mixture of 5.0 g of H2 (g) and 10.0 g of O2 (g) is ignited. Water forms according to the following addition reaction 2H2 (g) + O2 (g) 2 H2O (g) General Chemistry 1 Lab