3CuCl2(aq) + 2Al(s) + 3Cu(s) + 2AlCl3(aq) (Equation 1) 1. Find the atomic masses of copper...
Given the equation: 2Al(s) + 3CuCl2(aq) —> 3Cu(s) + 2AlCl3(aq) During an experiment 0.00293 moles of CuCl2 were used, and 0.064g of Al were left in the crucible. Calculate the theoretical moles and the theoretical mass of Al that should react.
The reducing agent in the reaction below is 3CuCl2(aq)+2Al(s) →3Cu(s)+2AlCl3(aq) a. Al3+ b. Cu2+ c. Al d. Cu
Experimental Yleld x 100% = Percent Yleld% (Equation 4) Theoretical Yleld Before you start the lab, it will be helpful to practices a few related problems. The information here is helpful when you complete your lab submission. ACTION REQUIRED Find the atomic masses of copper and chlorine, and the calculate the molar mass of CuCla. Keep THREE decimal places. Show all work and units: 1. Molar mass of Cu Molar Mass of Cl: Molar mass of CuCl If Sarah and...
Consider the following balanced equation: 6HCl(aq) + 2Al(s) → 3H2(g) + 2AlCl3(s) If 17.3 moles of HCl(aq) and 7.07 moles of Al(s) are allowed to react, and the percent yield is 71.8%, how many moles of AlCl3(s) will actually be produced?
a. 2Al(s)+3Cl2(g)→2AlCl3(s) You are given 19.0 g of aluminum and 24.0 g of chlorine gas.If you had excess aluminum, how many moles of aluminum chloride could be produced from 24.0 g of chlorine gas, Cl2? b. Determine the balanced chemical equation for this reaction. C8H18(g)+O2(g)→CO2(g)+H2O(g) c. 3H2(g)+N2(g)→2NH3(g) 1.08 g H2 is allowed to react with 10.3 g N2, producing 1.04 g NH3. What is the theoretical yield for this reaction under the given conditions? What is the percent yield for...
Preface: Aluminum foil was reacted will hydrochloric acid and copper 2 chloride. The copper solid from the reaction was placed on filter paper and dried. Data obtained from the lab is below Data Table Mass of Aluminum: 0.29g Mass of filter paper: 0.35g Mass of reacted filter paper: 0.49g Final mass of Copper: 0.11g 10mL of CuCl2: 0.100 CuCl2 molarity Volume of Copper Solution: ? Moles of Copper: 0.001g (0.1 molarity x 0.01 liters) Write an equation to represent the...
Data Mass of copper (II) chloride, CuCl2: 3,174g Mass of aluminum: 1.669g Mass of aluminum remaining after reaction: 0.530g Mass of aluminum that reacted: 1.139g Mass of filter paper and watchglass: 29.138g Mass of filter paper, watchglass, and copper: 32.829g Mass of copper recovered: 3.691 Questions (Show Work) Mole of CuCl2 dissolved Mole of copper (II) ions (Cu2+) initially in solution Mole of copper, Cu(s), expected to be formed Theoretical yield of copper in grams Percent yield of copper metal
Time Remaining:04:12:6 Consider the following balanced equation: 6HCl(aq) + 2Al(s) + 3H2(g) + 2AlCl3(S) 11 1.80x102 grams of HCl(aq) reacts with an excess of Al(s), and the percent yield is 53.6%, how many grams AlCl3(s) will actually be produced? 2.76x109 3.54x1099 9.88x1099 1.18*109 5.02*1099 Use the slider to rate your confidence on this question 100 Not at all confident Very confident
Question 3 [20 points 1. Copper sulfide is produced when copper and sulfur are heated together Use the data below, obtained after the heating process, to determine the empirical formula of this compound. Molar masses (e/mol) c S 32.06. 18 points) befor 1 Mass of crucible cover copper (B) 2 Mass of crucible + cover (g) 3 Mass of copper (B) 4 Mass of crucible cover + copper sulfide at constant weight (8)40.23 S Mass of copper sulfide (8) 6...
1.) Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. 2Al(s) + 6HCl(aq) -> 2AlCl3(aq) + 3H2(g) What mass of H2(g) is required from the reaction of 0.75 g of Al(s) with excess hydrochloric acid? 2.) The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). What mass of water is required for the formation of 175 grams of...