Domanda del libro di testo
Using values from Appendix C, calculate the value of H for each of the following reactions: (a) NiO(s) + 2 HCl(g) → NiCl2(s) + H2O(g)
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Ch.5 - Thermochemistry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 5, Problema 74
Many portable gas heaters and grills use propane, C3H8(g), as a fuel. Using standard enthalpies of formation, calculate the quantity of heat produced when 10.0 g of propane is completely combusted in air under standard conditions.
Guida verificata passo dopo passo1
Identify the balanced chemical equation for the combustion of propane: \( \text{C}_3\text{H}_8(g) + 5\text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 4\text{H}_2\text{O}(l) \).
Determine the standard enthalpies of formation (\( \Delta H_f^\circ \)) for each substance involved in the reaction: \( \text{C}_3\text{H}_8(g) \), \( \text{O}_2(g) \), \( \text{CO}_2(g) \), and \( \text{H}_2\text{O}(l) \).
Use the formula for the standard enthalpy change of the reaction: \( \Delta H_{rxn}^\circ = \sum \Delta H_f^\circ (\text{products}) - \sum \Delta H_f^\circ (\text{reactants}) \).
Calculate the moles of propane in 10.0 g using its molar mass: \( \text{moles of } \text{C}_3\text{H}_8 = \frac{10.0 \text{ g}}{\text{molar mass of } \text{C}_3\text{H}_8} \).
Multiply the moles of propane by the \( \Delta H_{rxn}^\circ \) to find the total heat produced during the combustion.
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Combustion Reaction
A combustion reaction is a chemical process in which a substance reacts rapidly with oxygen, producing heat and light. In the case of propane (C3H8), the combustion reaction involves its reaction with oxygen to produce carbon dioxide and water. Understanding this reaction is crucial for calculating the heat released during combustion.
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02:24
Combustion Apparatus
Standard Enthalpy of Formation
The standard enthalpy of formation (ΔHf°) is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. This value is essential for calculating the heat produced in a reaction, as it allows us to determine the total energy change by using the enthalpies of the reactants and products involved in the combustion of propane.
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02:34Enthalpy of Formation
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It is vital for determining the amount of heat produced from a specific mass of propane, as it allows us to convert grams of propane to moles and relate it to the heat released using the standard enthalpy of combustion.
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01:16Stoichiometry Concept
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