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1. What is stoichiometry?
2. For each equation, write all possible mole ratios.
a. 2HgO(s) → 2Hg(l) + O2(g)
b. 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l)
3. How is a mole ratio used in stoichiometry?
1. Balance the following equation. Then, given the moles of reactant or product below, determine the corresponding amount in moles of each of the other reactants and products.
NH3 + O2 → N2 + H2O
a. 4 mol NH3
b. 4 mol N2
c. 4.5 mol O2
2. One reaction that produces hydrogen gas can be represented by the
following unbalanced chemical equation:
Mg(s) + HCl(aq) → MgCl2(aq) + H2(g)
a. What mass of HCl is consumed by the reaction of 2.50 moles of magnesium?
b. What mass of each product is produced in part (a)?
1. Carbon disulfide burns in oxygen to yield carbon dioxide and sulfur dioxide according to the following chemical equation.
CS2(l) + 3O2(g) → CO2(g) + 2SO2(g)
a. If 1.00 mol CS reacts with 1.00 mol O2 identify the limiting reactant.
How many moles of excess reactant remain?
How many moles of each product are formed?
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