We will now extend our knowledge with its essentials with the prepared activities that expound everything wehave learned in the previous lessons.ACTIVITY 4HOW MUCH AM I FOR THE SECOND TIME?Stoichiometry deals with the amounts of reactants and products in a chemical reaction. It involves conversionof amounts of either reactant or product using mole method. In this activity, we will apply the concept of stoichiometryto look for the amounts of reactants and products in a chemical reaction using gas laws.Let us answer the given problems below.DIRECTION: Read, understand, and solve the following problems in gas stoichiometry. SHOW YOUR SOLUTION1. The equation for the metabolic breakdown of glucose (C6H1206) is the same as the equation for thecombustion of glucose in air:C6H1206(s) + 602(g) → 6CO2(g) + 6H20(1)Calculate the volume of CO, produced at 45 °C and 3.40 atm when 6.50 g of glucose is used up in thereaction. 2. Consider the formation of nitrogen dioxide from nitric oxide and oxygen:2NO(g) +O2(g) → 2NO2(g)If 10.0 L of NO are reacted with excess of O2 at STP, what is the volume in liters of NO2 produced?3. In alcohol fermentation, yeast converts glucose to ethanol and carbon dioxide:C6H12O6(s) → 2C2H5OH(I) +2CO2(g)If 6.87 g of glucose are reacted with and 1.55 L of CO2 gas are collected at 293 K and 0.975 atm, what is thepercent yield of the reaction?

Answered: 1. The equation for the metabolic…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter7: Chemical Reactions: An Introduction

Section: Chapter Questions

Problem 50A

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Acetylene gas, C2H2 , is used in welding because it generates an extremely hot flame when it is combusted with oxygen. The heat generated is sufficient to melt the metals being welded together. Carbon dioxide gas and water vapor are the chemical products of this reaction. Write the unbalanced chemical equation for the reaction of acetylene with oxygen.
Classify each of the following statements as true or false: a Coefficients in a chemical equation express the molar proportions among both reactants and products. b A stoichiometry problem can be solved with an unbalanced equation. c In solving a stoichiometry problem, the change from quantity of given substance to quantity of wanted substance is based on masses. d Percentage yield is actual yield expressed as a percentage of ideal yield. e The quantity of product of any reaction can be calculated only through the moles of the limiting reactant. f rH is positive for an endothermic reaction and negative for an exothermic reaction.
Nitrogen (N2) and hydrogen (H2)react to form ammonia (NH3). Consider the mixture of N2 and H2 in a closed container as illustrated below: Assuming the reaction goes to completion, draw a representation of the product mixture. Explain how you arrived at this representation.
Acetylene gas (C2H2) is often used by plumbers, welders, and glass blowers because it burns in oxygen with an intensely hot flame. The products of the combustion of acetylene are carbon dioxide and water vapor. Write the unbalanced chemical equation for this process.
Apply When a campfire begins to die down and smolder, you can rekindle the flame by fanning the fire. Explain, in terms of stoichiometry, why the fire again begins 10 flare up when fanned.
When elemental phosphorus, P4, burns in oxygen gas, it produces an intensely bright light, a great deal of heat, and massive clouds of white solid phosphorus(V) oxide (P2O5) product. Given these properties, it is not surprising that phosphorus has been used to manufacture incendiary bombs for warfare. Write the unbalanced equation for the reaction of phosphorus with oxygen gas to produce phosphorus(V) oxide.
Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.
A product weighing 14.37g was isolated from a reaction. The amount of product possible according to a calculation was 17.55g. What was the percentage yield?
What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?

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1. The equation for the metabolic breakdown of glucose (C6H1206) is the same as the equation for the combustion of glucose in air: C6H1206(s) + 6O2(g) → 6CO2(g) + 6H20(I) Calculate the volume of CO2 produced at 45 °C and 3.40 atm when 6.50 g of glucose is used up in the reaction.