Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reactionis:2 Mg (s)+ O2 2 Mg0 (s) When 10.1 g of Mg are allowed to react with 10.5 g of O2. 15.0 g of MgO are collected.Part ADetermine the limiting reactant for the reaction.Express your answer as a chemical formula.ANSWER:Part BDetermine the theoretical yield for the reaction.ANSWER:m3DPart CDetermine percent yield for the reaction.ANSWER:percent yieldExercise 8.40: Problems - Mass-to-Mass ConversionsConsider the following balanced equation for the combustion of butane, a fuel often used in lighters.2 C4H10 (9) +13 O2 (g) 8 CO2 (g) + 10 H2O (g) Complete the following table, showing the appropriate masses ofreactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react withthe given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses ofeach reactant to make that amount of product, as well as the mass of the other product that is formed.Mass C4H10 Mass O2 Mass CO2 Mass H2O1.11 g5.72 g18.12 g9.64 g192 mg168 mg

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Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reac is: 2 Mg (s) +O2 (9) -2 MgO (s) When 10.1 g of Mg are allowed to react with 10.5 g of O2. 15.0 g of MgO are collec Part A Determine the limiting reactant for the reaction. Express your answer as a chemical formula. ANSWER: Part B Determine the theoretical yield for the reaction. ANSWER: m%3D Part C Determine percent yield for the reaction. ANSWER: percent yield =

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reac is: 2 Mg (s) +O2 (9) -2 MgO (s) When 10.1 g of Mg are allowed to react with 10.5 g of O2. 15.0 g of MgO are collec Part A Determine the limiting reactant for the reaction. Express your answer as a chemical formula. ANSWER: Part B Determine the theoretical yield for the reaction. ANSWER: m%3D Part C Determine percent yield for the reaction. ANSWER: percent yield =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction
is:
2 Mg (s)+ O2 2 Mg0 (s) When 10.1 g of Mg are allowed to react with 10.5 g of O2. 15.0 g of MgO are collected.
Part A
Determine the limiting reactant for the reaction.
Express your answer as a chemical formula.
ANSWER:
Part B
Determine the theoretical yield for the reaction.
ANSWER:
m3D
Part C
Determine percent yield for the reaction.
ANSWER:
percent yield
Exercise 8.40: Problems - Mass-to-Mass Conversions
Consider the following balanced equation for the combustion of butane, a fuel often used in lighters.
2 C4H10 (9) +13 O2 (g) 8 CO2 (g) + 10 H2O (g) Complete the following table, showing the appropriate masses of
reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with
the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of
each reactant to make that amount of product, as well as the mass of the other product that is formed.
Mass C4H10 Mass O2 Mass CO2 Mass H2O
1.11 g
5.72 g
18.12 g
9.64 g
192 mg
168 mg

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