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Chemical Reactions: Stoichiometry and Metals

1. Calculate the molar mass of the following compounds:
a. sodium selenide
b. Palladium (II) hydroxide

2. Calculate the number of grams in each of the following compounds:
a. 4.0 moles of CaCl2(s)
b. 0.467 moles of (NH4)CO3(s), baking powder

3. Calulate the number of moles in each of the following compounds:
a. 150.0 g of NaBr (s)
b. 60.0g of ZnS(s)

4. Using the balanced chemical equation below, answer the following questions regarding mole relationships:
C3H8(g) + 5O2(g) -->3CO2(g) + 4H2O(g)
a.What are the mole-mole factors or molar rations of the following:
i. Propane to oxygen -->
ii. Water to carbon dioxide ->
iii. Carbon dioxide to oxygen -->
b.How many mole of oxygen gas are required to completely combust 7.0 moles of propane gas?
c.How many moles of carbon dioxide gas are produced from the burning of propane gas in the presence of 15.0 moles of oxygen gas?

5. Using the balanced chemical reaction below, answer the following questions regarding stoichiometry.

2K(s) + Zn(NO3)2(aq) --> Zn(s) + 2KNO3(aq)

a. Determine the mass of zinc metal produced from the reaction 6.0 moles of potassium metal in an excess solution of zinc nitrate.
b. Determine the number of moles of zinc nitrate solution required to react completely with 150.0g of potassium metal.
c. What mass of zinc metal will be produced from the reaction of 300.0 g of Zn(NO3)2 with an excess of potassium metal?

Solution Summary

The following problem helps with various physical chemistry problems. Concepts covered involve molar mass, stoichiometry and metals.