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11 Dec 2019

For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants.
2Al(s)+3Cl2(g)â2AlCl3(s)

1) 7.7 g Al, 24.4 g Cl2

Express your answer using three significant figures.

2)0.230 g Al, 1.15 g Cl2

Express your answer using three significant figures.

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13 Dec 2019

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For the reaction shown, compute the theoretical yield of the product in moles for each of the initial quanities of reactants. Ti(s)+ 2Cl2(g)=TiCl4(s) A) 2 mol Ti, 2 mol Cl2 express your answer using two significant figures. B) 5 mol Ti, 9 mol Cl2 express your answer using two significant figures. C) 0.483 mol Ti, 0.911 mol Cl2 express your answer using three significant figures. D) 12.4 mol Ti, 15.8 mol Cl2 express your answer using three significant figures

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction:

2Al(s)+3Cl2(g)â2AlCl3(s)

You are given 19.0 g of aluminum and 24.0 g of chlorine gas.

If you had excess chlorine, how many moles of of aluminum chloride could be produced from 19.0 g of aluminum? Express your answer to three significant figures and include the appropriate units.

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For the reaction shown, compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.

Ti(s)+2F2(g)âTiF4(s)

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Part B. Express your answer using two significant figures.

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Part C

0.236 g Ti, 0.286 g F2

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