chem 9 3

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 10.0 g of aluminum.

_____ Al(s) + _____ I₂(s) → _____ Al₂I₆(s)

0.556 mol

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq) in the following reaction?

BCl₃(g) + 3 H₂O(l) → 3 HCl(aq) + B(OH)₃(aq)

a.) 0.823 mol

b.) 0.0914 mol

c.) 0.655 mol

d.) 10.9 mol

e.) 0.274 mol

b.) 0.0914 mol

Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is the stoichiometric coefficient for sulfuric acid when the chemical equation is balanced using the lowest whole-number stoichiometric coefficients?

3

The balanced chemical equation for the reaction between PCl₅ and water is given below. If 3.45 moles of HCl are produced, how many moles of water reacted?

PCl₅ (aq) + 4 H₂O (l) → H₃PO₄ (aq) + 5 HCl (aq)

2.76 mol

Which is true of the reaction shown below?

Two molecules of Substance Y will be left over when this reaction goes to completion.

If 0.654 g of zinc metal reacts with 0.321 g of yellow powered sulfur, what is the mass of the zinc sulfide produced?

0.975 g

Chemical equations are balanced in order to obey the law of:

mass conservation.

If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to produce 42.0 g of oxygen?

2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)

165 g

When 10.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced. Using the following balanced equation, calculate the percent yield for the reaction?

Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g)

27.1%

What is the percent yield if the theoretical yield for a reaction was 156 g and 122 g of the product was actually made?

78.2%

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 5.00 g of dinitrogen monoxide decomposes?

1.82 g

What is the sum of the coefficients when the following equation is balanced using the lowest whole-numbered coefficients?

_____ PH3(g) + _____ O2(g) → _____ P4O10(s) + _____ H2O(g)

19

How many grams of H2O will be produced if 750 grams of Fe are produced?

__ H2 (g) + __ Fe3O4 (s) → __ H2O (g) + __ Fe (s)

322 g

Balance the chemical equation given below, and determine the number of grams of MgO needed to produce 15.0 g of Fe2O3.

_____ MgO(s) + _____ Fe(s) → _____ Fe2O3(s) + _____ Mg(s)

11.4 g

How many grams of the excess reagent are left over when 6.00 g of CS2 gas react with 10.0 g of Cl2 gas in the following reaction:

CS2(g) + 3 Cl2(g) → CCl4(l) + S2Cl2(l)

2.42 g

How many moles of CuO can be produced from 0.450 mol of Cu2O in the following reaction?

2 Cu2O(s) + O2(g) → 4 CuO(s)

0.900 mol

What is the molar mass of Co(NO3)2?

183 g/mol

Which one of the following contains 35% carbon by mass?

CH3F

What is the ratio of moles of oxygen used to moles of CO produced in the following reaction?

2 CO(g) + O(g) → 2 CO(g)

1:2

Consider the following equation:

4NH4 + 5O2 → 4 NO + 6H2O

How many moles of water are produced when 2 moles of NH4 react with excess oxygen gas?

3 mol

How many grams of calcium chloride are needed to produce 10.0 g of potassium chloride?

CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq)

7.44 g

What is the oxidation number change for the iron atom in the following reaction?

2 Fe2O3 (s) + 3 C(s) → 4 Fe(s) + 3 CO2(g)

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