For the following reaction for the synthesis of phosphorous acid: (5pts) ___PCl3(l) + ___H2O(l)  ___H3PO3(aq) + ___HCl(aq)

  1. For the following reaction for the synthesis of phosphorous acid: (5pts)

___PCl3(l) + ___H2O(l)  ___H3PO3(aq) + ___HCl(aq)

1.1. Balance the equation:

1.2. Determine how many moles of H2O are required to react completely with

4.90 moles phosphorus trichloride:

1.3. Determine how many moles of phosphorous acid are formed from 4.90 moles phosphorus trichloride (assume more than enough water present):

1.4. Determine how many moles of hydrochloric acid are formed from 4.90 moles phosphorus trichloride (assume more than enough water present):

1.5. Suppose we start the reaction with 100.0 g of phosphorus trichloride (assume more than enough water present), what mass (in g) of phosphorous acid can be synthesized:

Name_______________________________________________ Date:_______

  1. The reaction used for the synthesis of aspirin is shown below. In this reaction, an excess of acetic anhydride (C4H6O3) is added to a measured mass of salicylic acid (C7H6O3) in the presence of a catalyst. The products of the reaction are acetylsalicylic acid, aka aspirin (C9H8O4) and acetic acid (C2H4O2).

2.1. True or False:

This is a balanced chemical equation

2.2. Calculate the molar masses of all reactants and products (pay attention to significant figures:

Compound Chemical Formula Molar Mass (g/mol)
Salicylic acid
Acetic anhydride
Aspirin
Acetic acid

8

pts

2.3. What mass (in g) of acetic anhydride is required to completely react with

25.0 g salicylic acid?

2.4. The protocol in the lab calls for starting the reaction using 25.0 g salicylic acid and 32.0 g acetic anhydride.

2.4.1. Find the limiting reactant

2.4.2. Identify the excess reactant

Name_______________________________________________ Date:_______

2.4.3. Calculate the theoretical yield of aspirin (in g)

2.4.4. Assume that after completing the reaction we collected 29.5 g of aspirin.

Calculate the percent yield for the reaction.

  1. 1te the molarity of a solution made by dissolving 3.2 mol of glucose (C6H12O6) to obtain 1.10 L solution

  2. What volume of 0.200M ethanol solution contains 1.22 mol ethanol?

BONUS QUESTION:

A chemist wants to make 7.2L of 0.350 M CaCl2 solution. What mass of CaCl2 in grams should the chemist use?

1 pt

1 pt

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