1. How many moles of Al are necessary to form 76.2 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s) ?
____mol
2. What is the mass in grams of H₂ that can be formed from 48.2 grams of NH₃ in the following reaction? 2 NH₃(g) → 3 H₂(g) + N₂(g)
____g
3. What is the difference between actual yield and theoretical yield?
A) Actual yield has to do only with the reactants of a reaction, and theoretical yield has to do only with the products of a reaction.
B) Actual yield is how much is actually produced in a reaction (it has to be given or measured), and theoretical yield is a calculation that has to be done.
C) Actual yield is how much the reaction produces, and theoretical yield is how much a reaction consumes.
D) Actual yield has to do with how much you can actually get out of a reaction, and theoretical yield is how much you can get out of a reaction if you have maximum starting materials.
4. 200.0 mL of a 0.900 M solution of KCl is diluted to 600.0 mL. What is the new concentration of the solution?
____M
5. A student combined 37.2 mL of 1.69 M KMnO₄ solution with 15.70 mL of a 0.891 M KMnO₄ solution. Calculate the concentration of the final solution.
____M
6. How many moles of CH₃OH are there in 150.0 mL of 0.495 M CH₃OH?
____mol
7. What is the concentration of lithium ions in 0.110 M Li₂HPO₄?
____M
8. How many mL of 0.200 M KBr would be required to make a 0.0625 M solution of KBr when diluted to 175.0 mL with water?
____mL
9. If 28.7 g of C₂H₅OH (MM = 46.07 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of C₂H₅OH in the resulting solution?
____M
10. To what volume (in mL) would you need to dilute 25.0 mL of a 1.45 M solution of KCl to make a 0.0375 M solution of KCl?
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