Ch.6 - Thermochemistry WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction:2 CO(g) + O2(g) → 2 CO2(g)∆H for this reaction is −135.28 kcal. How much heat would be released if 18.0 moles of carbon monoxide reacts with 12.0 moles of oxygen?1. 811 kcal2. 1623 kcal3. 2705 kcal4. 216 kcal5. 1218 kcal 6. 29,160 kcal7. 406 kcal

Solution: Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction:2 CO(g) + O2(g) → 2 CO2(g)∆H for this reaction is −135.28 kcal. How much heat would be released if 18.0 moles of car

Problem

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction:

2 CO(g) + O2(g) → 2 CO2(g)

∆H for this reaction is −135.28 kcal. How much heat would be released if 18.0 moles of carbon monoxide reacts with 12.0 moles of oxygen?

1. 811 kcal

2. 1623 kcal

3. 2705 kcal

4. 216 kcal

5. 1218 kcal 

6. 29,160 kcal

7. 406 kcal

Solution

We’re being asked to determine the heat (q) released by the given reaction:

2 CO(g) + O2(g)  2 CO2(g); ΔH = –135.28 kcal


The problem states that 18.0 moles of CO react with 12.0 moles of O2. We first need to determine the limiting reactant.


Recall that the limiting reactant is the reactant that forms the less amount of product. This is because once the limiting reactant is all used up, the reaction can no longer proceed and make more products.


We need to perform a mole-to-mole comparison between each reactant and CO2.


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