Derivation Look up the values of E° for the following half-cell reactions. Ag+ + e - Ag AgBr + e - Ag + Br Describe how you would use these values to determine the solubility product (Ksp) of AgBr at 25.0°C. Step 1 of 4 Recall and write the equilibrium expression for the Ksp of AgBr. (Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPad O Help Greek {Ag+}{Br-} {Ag+}{Br-} Your answer differs too much from the expected answer to provide useful feedback. Submit

Derivation Look up the values of E° for the following half-cell reactions. Ag+ + e - Ag AgBr + e - Ag + Br Describe how you would use these values to determine the solubility product (Ksp) of AgBr at 25.0°C. Step 1 of 4 Recall and write the equilibrium expression for the Ksp of AgBr. (Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPad O Help Greek {Ag+}{Br-} {Ag+}{Br-} Your answer differs too much from the expected answer to provide useful feedback. Submit

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Predict reaction and calculate Eº, cell = A voltaic cell is constructed from a standard Zn²+ | Zn half cell (E° red -0.763V) and a standard Mn2+ | Mn half cell (E° red = -1.180V). What is the spontaneous reaction that takes place, and what is the standard cell potential? Spontaneous cell reaction: Write a balanced equation using the smallest integer coefficients possible. + from standard reduction potentials. Standard cell potential: V. +
Consider the following reaction and their reduction potential values: Cu+ + Ni2+ —> Cu2+ + Ni (Format: half reaction, E⁰) Cu2+ + e- —> Cu+, 0.15 V Ni2+ + 2e- —> Ni, -0.25 V What is the overall cell potential and is the overall reaction spontaneous?
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Using the provided standard reduction potentials, which of the following cells is an example of a Galvanic cell? Recall the general form of cell notation. Note: The one with smaller value is the anode. -1.5 -1.0 -0.5 0.0 +0.5 +1.0 +1.5 Zn2+/Zn Sn2+/Sn Ag*/Ag Au*/Au Fe2+/Fe Cu2+/Cu
What is the standard cell potential for the reaction below? Enter your answer with two decimal places and no units. Mg(s) + Br2() Mg2+(aq) + 2 Br"aq) The standard reduction potential is -2.37 V for the Mg2+/Mg half-cell and +1.09 V for the Bro/Br half-cell. Enter your answer in decimal format using two decimal places, (value + 2%).
Use the given galvanic cell notation below to answer the following questions. 2+ Sn (s) | Sn²+ (aq) || Ti+ (aq)| Ti (s) a) Write the oxidation half reaction. Balance and include states. b) Write the reduction half reaction. Balance and include states. c) Write the overall cell reaction. Balance and include states. d) Identify the anode and cathode. Label your answers a), b), c), d).
Silver (Ag) is observed to corrode in HCl (1M activity) in aerated condition. 1) Write the anodic and cathodic half reactions. Write ½ reactions as reduction reactions. 2) What are the standard potentials of the ½ reactions Following the previous question, write the overall reaction? 3) What is the overall potential difference?
In a voltaic cell, one compartment/electrode is a Ag*(0.600 M) | Ag(s) half-cell, the other is a standard hydrogen electrode (saturated hydrogen gas on Pt metal) immersed in a 0.040 M HCI solution. a. Write the line notation for the cell, including all concentrations, partial pressures and states. Write the two half-reactions (clearly indicate if it is the anode or cathode) and the overall reaction of this voltaic cell. b. Calculate Eo cell - C. Calculate Ecell at 25 °C. d. Calculate Ecell at 25 °C if the hydrogen electrode is immersed in a buffer solution containing 0.064 M acetic acid, CH3COOH (MM = 60.05 g-mol-1) and 0.376 M sodium acetate, NaCH3COO (MM = 82.03 g-mol-1). Use pka (CH3COOH) = 4.8. %3D %3D %3D
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Calculate e° values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLV2 MindTap Reader. You should not use the OWLV2 References' Tables to answer this question as the values will not match.) a. Cr*+ (ag) + Cl2 (g) = Cr2O,²- (ag) + Cl¯ (ag) V b. Cd²+ (ag) + Ba(s) = Ba2+ (aq) + Cd(s) V
9. Using the appropriate half-cell reactions, and assuming 7. = product of AgCl at 25°C: AgCl(s) Ag' (aq) + Cl(aq) a) 5.21 × 10-13 b) 1.68 × 10-10 1.85 × 10-10 1, calculate the solubility d) 1.56× 10-1 0.100