4. Solving a mass-to-mass problem requires the four steps listed below. The equations in the boxesshow how the four steps are used to solve an example problem. After you have studied the example,solve the problems below, using the four steps.Example problem: How many grams of carbon dioxide are produced when 20.0 g acetylene (C₂H₂) is burned?Step 1 Write a balanced chemical equation for the reaction.Step 2 Determine the number of moles of the known substance, usingmass-to-mole conversion.Step 3 Determine the number of moles of the unknown substance, usingmole-to-mole conversion.Step 4 Determine the mass of the unknown substance, using mole-to-massconversion.neaysrilSolution2C₂H2(g) + 5O2(g) → 4CO2(g) + 2H₂O(g)1 mol C₂H₂26.04 g C₂H₂SF4+H₂O → SO₂ + HF20.0 g C₂H₂ x= 0.768 mol C₂H₂0.768 molC₂H₂ x= 1.54 mol CO₂1.54 mol= 67.8 g CO₂4 mol CO₂2 molC₂H₂a) In a blast furnace, iron and carbon monoxide are produced from the reaction of iron(III) oxide (Fe2O3)and carbon. How many grams of iron are formed when 150 g iron(III) oxide reacts with an excess ofcarbon?of wollx44.01 g CO₂cure adImoleoFe₂O3+ C Fe + COb) Solid sulfur tetrafluoride (SF4) and water react to form sulfur dioxide and an aqueous solution ofhydrogen fluoride. How many grams of water are necessary for 20.0 g sulfur tetrafluoride to reactcompletely?

Note: As per the guidelines solution of question 4(a) has been made and for the expert solution of…

a) In a blast furnace, iron and carbon monoxide are produced from the reaction of iron(III) oxide (Fe2O3) and carbon. How many grams of iron are formed when 150 g iron(III) oxide reacts with an excess of carbon? Fe2O3+ C Fe + CO

a) In a blast furnace, iron and carbon monoxide are produced from the reaction of iron(III) oxide (Fe2O3) and carbon. How many grams of iron are formed when 150 g iron(III) oxide reacts with an excess of carbon? Fe2O3+ C Fe + CO

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

4. Solving a mass-to-mass problem requires the four steps listed below. The equations in the boxes
show how the four steps are used to solve an example problem. After you have studied the example,
solve the problems below, using the four steps.
Example problem: How many grams of carbon dioxide are produced when 20.0 g acetylene (C₂H₂) is burned?
Step 1 Write a balanced chemical equation for the reaction.
Step 2 Determine the number of moles of the known substance, using
mass-to-mole conversion.
Step 3 Determine the number of moles of the unknown substance, using
mole-to-mole conversion.
Step 4 Determine the mass of the unknown substance, using mole-to-mass
conversion.
neay
sril
Solution
2C₂H2(g) + 5O2(g) → 4CO2(g) + 2H₂O(g)
1 mol C₂H₂
26.04 g C₂H₂
SF4+H₂O → SO₂ + HF
20.0 g C₂H₂ x
= 0.768 mol C₂H₂
0.768 molC₂H₂ x
= 1.54 mol CO₂
1.54 mol
= 67.8 g CO₂
4 mol CO₂
2 molC₂H₂
a) In a blast furnace, iron and carbon monoxide are produced from the reaction of iron(III) oxide (Fe2O3)
and carbon. How many grams of iron are formed when 150 g iron(III) oxide reacts with an excess of
carbon?
of woll
x
44.01 g CO₂cure ad
Imoleo
Fe₂O3+ C Fe + CO
b) Solid sulfur tetrafluoride (SF4) and water react to form sulfur dioxide and an aqueous solution of
hydrogen fluoride. How many grams of water are necessary for 20.0 g sulfur tetrafluoride to react
completely?

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