Limiting/Excess Reagent Stoichiometry

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Presentation transcript:

Limiting/Excess Reagent Stoichiometry Alyssa Armeni

16.7g of Li is reacted with 30.7g of S, how many grams of Li2S is produced? What is the limiting reagent? What is the excess reagent? How much excess will there be?

Draw a complete and Balanced Equation 2Li + S  Li2S

Draw a Column for Each Chemical 2Li S Li2S

Write One of the Amounts Given in the Appropriate Column 2Li S Li2S 16.7g

Convert the Amount Given into Moles 2Li S Li2S 16.7g

Find Moles for Each of the Other Chemicals Start with Given Moles In Each Other Column 2Li S Li2S 16.7g 2.41m

Create Fraction to Find Moles Numerator is Coefficient of that Column 2Li S Li2S 16.7g 2.41m

Finish Fraction to Find Moles Denominator is Coefficient of Given Column 2Li S Li2S 16.7g 2.41m

Draw a Line Under Your Work and Write the Second Amount Given Under the Appropriate Column Li2S 16.7g 2.41m 30.7g

Convert the Second Given into Moles 2Li S Li2S 16.7g 2.41m 30.7g

Get Rid of the Bigger Equation Since you can have moles in the same column, you can compare and get rid of the Excess reagent. 1.21 is bigger than .957, therefore the top is bigger and can be crossed out. 2Li S Li2S 16.7g 2.41m 30.7g X

Answer Since the top number was bigger, the given from that section is the excess reagent. Lithium was on the top so it has the excess amount. That makes the bottom given reagent, Sulfur, the limiting reagent.

Repeat the Work Done in the Top Row for the Bottom Row to Answer the Other Questions 2Li S Li2S 30.7g

Find Moles for Each of the Other Chemicals Start with Given Moles In Each Other Column 2Li S Li2S .957m 30.7g

Create Fraction to Find Moles Numerator is Coefficient of that Column 2Li S Li2S .957m 30.7g

Finish Fraction to Find Moles Denominator is Coefficient of Given Column 2Li S Li2S .957m 30.7g

Convert Back to Grams 2Li S Li2S .957m 30.7g

Verify the Law of Conservation of Mass 2Li S Li2S 13.3g 30.7g 44.0g 13.3g+30.7 44.0 44.0g = 44.0g

Answers 2 There were 44.0g of Li2S. In this reaction only 13.3g of Li were used, subtract this from the given, 16.7g. This gives you an excess amount of 3.4g

All Answers Together How many grams of Li2S is produced? 44.0g What is the limiting reagent? Sulfur What is the excess reagent? Lithium How much excess will there be? 3.4g