Lab: Limiting Reactant and Percent Yield Answers

Was this hypothesis supported in the lab?✔ yessomewhata littleno

separated from the copperaluminum✔ aqueous solutioncopper(II) chloride.

The molar mass of Cu is 63.55 g/mol. The number of grams of Cu produced in this reaction is 0.001230.00724✔ 4.9629.3.

Determined using stoichiometry: ✔ theoretical yieldexperimental yieldboth

The percent yield of a chemical reaction is theoretical yieldexperimental yield✔ both theoretical yield and experimental yield.

What could have accounted for a percent yield of less than 100% in this lab? Check all that apply.

During Trial 2, what allowed you to determine that aluminum was the limiting reactant? Check all that apply.

Which tool was used to collect the solid product of the chemical reaction?

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With this tool, the ✔ copperaluminumaluminum chloridewater could be

The balanced chemical equation for this lab is:3CuCl2(aq) + 2Al(s) 3Cu(s) + 2AlCl3(aq)If 10.5 g copper chloride react with 12.4 g aluminum, what is the limiting reactant?

Burning a candle is a combustion reaction that uses wax and oxygen to produce carbon dioxide, water, and energy. When you burn a candle down in an open room, the limiting reactant is oxygen✔ waxenergywater.

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Label each of the descriptions below as theoretical yield, experimental yield, or both.Calculated based on the chemical equation: ✔ theoretical yieldexperimental yieldboth

The percent yield of a chemical reaction is valuable to many industries. Low percent yields can result in the loss of large amounts of money. Which of the following would likely increase the percent yield of a reaction? Check all that apply.

The number of moles of Cu produced in this reaction is ✔ 0.0780.1180.3070.460.

When you place a glass over a candle and the flame goes out, the limiting reactant is ✔ oxygenwaxenergywater.

Measured directly: theoretical yield✔ experimental yieldboth

Determined experimentally: theoretical yield✔ experimental yieldboth