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(a)
Interpretation:
The reactant present in excess when 2.22 g of magnesium is heated to 3.75 g of nitrogen is to be identified.
Concept introduction:
The
1. Combination redox reaction
2. Decomposition redox reaction
3. Displacement redox reactions
Combination redox reactions are the reactions in which two or more reactants combine to form a single product. In displacement redox reactions, substances on both sides of the equation remain the same but the atoms exchange places in order to form the product while in decomposition reaction, one compound decomposes to form one or more product.
A limiting reagent is the one that is completely consumed in a
(a)
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Answer to Problem 4.116P
The reactant present in excess when 2.22 g of magnesium is heated to 3.75 g of nitrogen is N2.
Explanation of Solution
Magnesium reacts with nitrogen molecule to form magnesium nitride (Mg3N2). The balanced chemical equation of the redox reaction is:
3Mg(s)+N2(g)→Mg3N2(s)
Three moles of Mg combine with one mole of N2 to give two moles of Mg3N2.
The molecular mass of Mg is 24.31 g/mol.
The formula to calculate moles of Mg3N2 when Mg is limiting reagent is:
Moles of Mg3N2=[(mass of Mg(g)molecular mass of Mg(g/mol))(1 mol Mg3N23 mol Mg)] (1)
Substitute 2.22 g for mass of Mg and 24.31 g/mol for molecular mass of Mg in the equation (1).
Moles of Mg3N2=[(2.22 g24.31 g/mol)(1 mol Mg3N23 mol Mg)]=[(0.10037 mol)(1 mol Mg3N23 mol Mg)]=0.030440 mol
The molecular mass of N2 is 28.02 g/mol.
The formula to calculate moles of Mg3N2 when N2 is limiting reagent is:
Moles of Mg3N2=[(mass of N2(g)molecular mass of N2(g/mol))(1 mol Mg3N21 mol N2)] (2)
Substitute 3.75 g for the mass of N2 and 28.02 g/mol for molecular mass of N2 in the equation (2).
Moles of Mg3N2=[(3.75 g28.02 g/mol)(1 mol Mg3N21 mol N2)]=[(0.133832 mol)(1 mol Mg3N21 mol N2)]=0.13383 mol
Mg is limiting reagent in the reaction as the moles of Mg3N2 produced is less in this case as compared to when N2 is the limiting agent.
The reactant present in an excess concentration in the reaction is N2.
The reactant present in excess when 2.22 g of magnesium is heated to 3.75 g of nitrogen is N2.
(b)
Interpretation:
The moles of product formed when 2.22 g of magnesium is heated to 3.75 g of nitrogen
is to be calculated.
Concept introduction:
The redox reaction can be classified into three types depending upon the number of reactants and products as follows:
1. Combination redox reaction
2. Decomposition redox reaction
3. Displacement redox reactions
Combination redox reactions are the reactions in which two or more reactants combine to form a single product. In displacement redox reactions, substances on both sides of the equation remain the same but the atoms exchange places in order to form the product while in decomposition reaction, one compound decomposes to form one or more product.
A limiting reagent is the one that is completely consumed in a chemical reaction. The amount of product formed in any chemical reaction has to be in accordance with the limiting reagent of the reaction. The amount of product depends on the amount of limiting reagent since the product formation is not possible in the absence of it.
(b)
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Answer to Problem 4.116P
The moles of product formed when 2.22 g of magnesium is heated to 3.75 g of nitrogen is 0.030440 mol.
Explanation of Solution
Magnesium reacts with nitrogen molecule to form magnesium nitride (Mg2N3). The balanced chemical equation of the redox reaction is:
3Mg(s)+N2(g)→Mg3N2(s)
Magnesium is the limiting agent in the reaction.
Three moles of Mg combine with one mole of N2 to give two mole of Mg3N2.
The molecular mass of Mg is 24.31 g/mol.
The formula to calculate moles of Mg3N2 when Mg is limiting reagent is:
Moles of Mg3N2=[(mass of Mg(g)molecular mass of Mg(g/mol))(1 mol Mg3N23 mol Mg)] (1)
Substitute 2.22 g for the mass of Mg and 24.31 g/mol for molecular mass of Mg in the equation (1).
Moles of Mg3N2=[(2.22 g24.31 g/mol)(1 mol Mg3N23 mol Mg)]=[(0.10037 mol)(1 mol Mg3N23 mol Mg)]=0.030440 mol
The moles of product formed when 2.22 g of magnesium is heated to 3.75 g of nitrogen is 0.030440 mol.
(c)
Interpretation:
The mass of each reactant and product after the reaction is to be calculated.
Concept introduction:
The redox reaction can be classified into three types depending upon the number of reactants and products as follows:
1. Combination redox reaction
2. Decomposition redox reaction
3. Displacement redox reactions
Combination redox reactions are the reactions in which two or more reactants combine to form a single product. In displacement redox reactions, substances on both sides of the equation remain the same but the atoms exchange places in order to form the product while in decomposition reaction, one compound decomposes to form one or more product.
A limiting reagent is the one that is completely consumed in a chemical reaction. The amount of product formed in any chemical reaction has to be in accordance with the limiting reagent of the reaction. The amount of product depends on the amount of limiting reagent since the product formation is not possible in the absence of it.
(c)
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Answer to Problem 4.116P
The mass of Mg, N2 and Mg3N2 after the reaction are 0, 2.90 g and 3.07 g respectively.
Explanation of Solution
Magnesium is the limiting agent in the reaction. Hence, no moles of magnesium will be left after the completion of the reaction.
The molecular mass of Mg3N2 is 100.95 g/mol.
The formula to calculate the mass of Mg3N2 is:
Mass of Mg3N2=[(moles of Mg3N2(mol))(molecular mass of Mg3N2(g/mol))] (3)
Substitute 0.030440 mol for moles of Mg3N2 and 100.95 g/mol for molecular mass of Mg3N2 in the equation (3).
Mass of Mg3N2=[(0.030440 moll)(100.95 g/mol)]=3.07292 g≈3.07 g
The formula to calculate the mass of N2 reacted is:
Mass of N2 reacted=[(mass of Mg(g)molecular mass of Mg(g/mol))(1 mol N23 mol Mg)molecular mass of N2(g/mol)] (4)
Substitute 2.22 g for the mass of Mg, 24.31 g/mol for molecular mass of Mg and 28.02 g/mol for molecular mass of N2 in the equation (4).
Mass of N2 reacted=[(2.22 g24.31 g/mol)(1 mol N23 mol Mg)(28.02 g/mol)]=0.852933 g
The formula to calculate the mass of remaining N2 is:
Remaining N2=(Initial amount of N2)−(Reacted amount of N2) (5)
Substitute 3.75 g for the initial mass of N2 and 0.852933 g for the reacted mass of N2 in the equation (5).
Remaining N2=(3.75 g)−(0.852933 g)=2.897067 g≈2.90 g
The mass of Mg, N2 and Mg3N2 after the reaction are 0, 2.90 g and 3.07 g respectively.
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Chapter 4 Solutions
Chemistry: The Molecular Nature of Matter and Change
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