- 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:
- 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)
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
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.
- 1te the molarity of a solution made by dissolving 3.2 mol of glucose (C6H12O6) to obtain 1.10 L solution
What volume of 0.200M ethanol solution contains 1.22 mol ethanol?
A chemist wants to make 7.2L of 0.350 M CaCl2 solution. What mass of CaCl2 in grams should the chemist use?