Domanda del libro di testo
Consider the unbalanced equation: (b) Use the data in Appendix B and ΔG°f for IO3-(aq)= -128.0 kJ/mol to calculate ΔG° for the reaction at 25 °C.
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Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium
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
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McMurry 8th EditionCh.18 - Thermodynamics: Entropy, Free Energy & EquilibriumProblema 141a
McMurry 8th EditionCh.18 - Thermodynamics: Entropy, Free Energy & EquilibriumProblema 141aCapitolo 18, Problema 141a
Consider the unbalanced equation: (a) Balance the equation for this reaction in basic solution.
Guida verificata passo dopo passo1
Identify the elements that are not balanced in the given chemical equation.
Assign oxidation numbers to each element in the reaction to identify the elements undergoing oxidation and reduction.
Write the half-reactions for the oxidation and reduction processes.
Balance each half-reaction for mass and charge. Start by balancing all elements except hydrogen and oxygen, then balance oxygen atoms by adding H2O, and hydrogen atoms by adding H+.
Since the reaction occurs in a basic solution, add OH- to both sides of the equation to neutralize the H+ ions, forming water. Combine and simplify the half-reactions to get the balanced equation.
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Balancing Chemical Equations
Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is crucial for obeying the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Balancing can be achieved by adjusting coefficients in front of the chemical formulas.
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Percorso guidato
01:32
Balancing Chemical Equations
Basic Solution
A basic solution is one where the pH is greater than 7, indicating a higher concentration of hydroxide ions (OH-) than hydrogen ions (H+). In balancing reactions in basic solutions, hydroxide ions and water are often added to neutralize any hydrogen ions produced during the reaction, which helps in achieving a balanced equation.
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Percorso guidato
01:04Balancing Basic Redox Reactions
Half-Reaction Method
The half-reaction method is a systematic approach to balancing redox reactions by separating the oxidation and reduction processes. Each half-reaction is balanced for mass and charge, and then combined to form the overall balanced equation. This method is particularly useful in basic solutions, where additional steps may be required to account for hydroxide ions.
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Percorso guidato
01:49Method 1 of Radioactive Half-Life
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Domanda del libro di testo
Consider the unbalanced equation: I2(s) → I-(aq) + IO3-(aq) (d) What pH is required for the reaction to be at equilibrium at 25°C when [I-] = 0.10M and [IO3-] = 0.50 M?
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Domanda del libro di testo
The lead storage battery uses the reaction: (b) Calculate ∆G for this reaction on a cold winter's day (10 °F) in a battery that has run down to the point where the sulfuric acid concentration is only 0.100 M.
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Domanda del libro di testo
A mixture of 14.0 g of N2 and 3.024 g of H2 in a 5.00 L container is heated to 400 °C. Use the data in Appendix B to calculate the molar concentrations of N2, H2, and NH3 at equilibrium. Assume that ∆H° and ∆S° are independent of temperature, and remember that the standard state of a gas is defined in terms of pressure.
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Domanda del libro di testo
Methanol (CH3OH) is made industrially in two steps from CO and H2. It is so cheap to make that it is being considered for use as a precursor to hydrocarbon fuels, such as methane (CH4):
Step 1. CO(g) + 2 H2(g) S CH3OH(l) ΔS° = - 332 J/K
Step 2. CH3OH1l2 → CH4(g) + 1/2 O2(g) ΔS° = 162 J/K
(k) Calculate an overall ΔG°, ΔH°, and ΔS° for the formation of CH4 from CO and H2.
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Domanda del libro di testo
Chloroform has ΔHvaporization = 29.2 kJ>mol and boils at 61.2 °C. What is the value of ΔSvaporization for chloroform?
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