Domanda del libro di testo
Calculate ∆G°rxn and K for each reaction. b. The reaction of Cr3+(aq) and Cr(s) to form Cr2+(aq). [The electrode potential of Cr2+(aq) to Cr(s) is -0.91 V.]
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Ch.19 - Electrochemistry
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 19, Problema 125
A sample of impure tin of mass 0.535 g is dissolved in strong acid to give a solution of Sn2+. The solution is then titrated with a 0.0448 M solution of NO3–, which is reduced to NO(g). The equivalence point is reached upon the addition of 0.0344 L of the NO3– solution. Find the percent by mass of tin in the original sample, assuming that it contains no other reducing agents.
Guida verificata passo dopo passo1
Identify the balanced chemical equation for the reaction between Sn^{2+} and NO_3^-: Sn^{2+} + 2 NO_3^- + 4 H^+ \(\rightarrow\) Sn^{4+} + 2 NO + 2 H_2O.
Calculate the moles of NO_3^- used in the titration using the formula: \(\text{moles of NO}\)_3^- = \(\text{molarity}\) \(\times\) \(\text{volume in liters}\).
Use the stoichiometry of the balanced equation to find the moles of Sn^{2+} that reacted. According to the equation, 1 mole of Sn^{2+} reacts with 2 moles of NO_3^-.
Calculate the mass of tin (Sn) that reacted using the moles of Sn^{2+} and the molar mass of tin (118.71 \(\text{ g/mol}\)).
Determine the percent by mass of tin in the original sample using the formula: \(\text{percent by mass}\) = \(\left\)( \(\frac{\text{mass of tin}\)}{\(\text{mass of sample}\)} \(\right\)) \(\times\) 100.
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Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this question, stoichiometry is essential for relating the moles of tin (Sn) to the moles of nitrate (NO3-) used in the titration, allowing for the determination of the mass of tin in the sample.
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Percorso guidato
01:16
Stoichiometry Concept
Titration
Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant to a solution until the reaction reaches its equivalence point, where stoichiometrically equivalent amounts of reactants have reacted. In this scenario, the titration of Sn2+ with NO3- allows for the calculation of the amount of tin present based on the volume and concentration of the nitrate solution used.
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Percorso guidato
03:04Acid-Base Titration
Percent by Mass
Percent by mass is a way to express the concentration of a component in a mixture or solution, calculated as the mass of the component divided by the total mass of the mixture, multiplied by 100. In this problem, after determining the mass of tin from the titration data, calculating the percent by mass involves comparing the mass of tin to the original mass of the impure sample, providing insight into the purity of the tin.
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Percorso guidato
00:38Mass Percent Calculation
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A metal forms the fluoride MF3. Electrolysis of the molten fluo- ride by a current of 3.86 A for 16.2 minutes deposits 1.25 g of the metal. Calculate the molar mass of the metal.
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Domanda del libro di testo
A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to H2(g), which bubles out of solution. What is the pH of the solution after 73 minutes?
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Domanda del libro di testo
An MnO2(s)/Mn2+(aq) electrode in which the pH si 10.24 is prepared. Find the [Mn2+] necessary to lower the potential of the half-cell to 0.00 V (at 25°C)
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