Domanda del libro di testo
Use the information in Table 9.2 to calculate ΔH° in kilojoules for the photosynthesis of glucose (C6H12O6) and O2 from CO2 and liquid H2O, a reaciton carried out by all green plants
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Ch.9 - Thermochemistry: Chemical Energy
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 9, Problema 116c
Use the data in Appendix B to find standard enthalpies of reaction in kilojoules for the following processes: (c) Fe2O3 (s) + 3 CO (g) → Fe(s) + 3 CO2(g)
Guida verificata passo dopo passo1
Identify the reactants and products in the given chemical reaction. For this reaction, the reactants are Fe2O3 (s) and CO (g), and the products are Fe (s) and CO2 (g).
Look up the standard enthalpy of formation (\(\Delta H_f^\circ\)) for each reactant and product in Appendix B. The values you need are for Fe2O3 (s), CO (g), Fe (s), and CO2 (g).
Write down the standard enthalpy of formation for each substance. Make sure to note the physical state (solid, liquid, gas) as it is crucial for accurate values.
Apply Hess's Law to calculate the standard enthalpy of reaction (\(\Delta H_{rxn}^\circ\)). Use the formula: \(\Delta H_{rxn}^\circ = \sum (\Delta H_f^\circ \text{ of products}) - \sum (\Delta H_f^\circ \text{ of reactants})\).
Substitute the standard enthalpies of formation into the equation and calculate the sum for the products and the reactants separately. Then, find the difference between these sums to get the standard enthalpy of reaction.
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Standard Enthalpy of Reaction
The standard enthalpy of reaction (ΔH°) is the change in enthalpy when reactants are converted to products under standard conditions (1 atm pressure and 25°C). It is a crucial concept in thermodynamics, allowing chemists to predict the heat absorbed or released during a chemical reaction. This value can be calculated using Hess's law or from standard enthalpies of formation.
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Enthalpy of Formation
Hess's Law
Hess's Law states that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps, regardless of the pathway taken. This principle allows for the calculation of enthalpy changes for reactions that are difficult to measure directly by using known enthalpy changes of related reactions. It emphasizes the state function nature of enthalpy.
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02:03Hess's Law
Enthalpy of Formation
The enthalpy of formation (ΔHf°) is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. These values are tabulated for many substances and are essential for calculating the standard enthalpy of reaction using the formula: ΔH° = ΣΔHf°(products) - ΣΔHf°(reactants). Understanding this concept is vital for thermodynamic calculations in chemistry.
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02:34Enthalpy of Formation
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Use the data in Appendix B to find standard enthalpies of reaction in kilojoules for the following processes: (b) 2 H2O2 (aq) → 2 H2O (l) + O2(g)
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Use the data in Appendix B to find standard enthalpies of reaction in kilojoules for the following processes: (a) C(s) + CO2(g) → 2 CO(g)
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