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30 May 2020

Copper can form two binary compounds with chlorine, and . It is known that of copper would need  of chlorine to form and the ratio of in is . What would be the mass of chlorine required to react with of to form ?

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Hubert Koch
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1 Sep 2020

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Related questions

1) What is the mass of silver that can be prepared from 1.40 g of copper metal?
Cu(s)+2AgNO3(aq)→Cu(NO3)2(aq)+2Ag(s)

2a) How many moles of chlorine gas react with 0.160 mol of metallic iron?

2b) How many moles of iron(III) chloride are produced?

2. Determine the mass of chlorine in the original sample as the difference in mass between the anhydrous sample (after drying in the crucible) and the mass of copper(1g). From the mass of chlorine, determine the moles of Cl. 3. Determine the experimental molar ratio of Cu:Cl. 4. In Step 12, describe the components involved in the reaction. What evidence is there for a chemical reaction? Describe where the reaction is occurring on the molecular level. 5. a. Without attempting to measure the mass of the aluminum, consider the reaction that occurs in step 12, what would an increase in the aluminum mass indicate? b. What would a decrease in the aluminum mass indicate?

step 12. React the copper chloride solution to generate elemental copper.

a. Obtain a piece of aluminum wire. If the wire is dull, sand it with the sandpaper until shiny.b. Coil the wire loosely around your index and middle fingers. Fewer coils arebetter.c. Place the wire in the beaker of copper chloride solution so that it is completely immersed. It may need to be pushed down with a stir rod. Make sure the reaction goes to completion before continuing.


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