A group of students were tasked to perform the metal coupling of iron nail similar to Experiment 3: Corrosion of Metals. They were given two metals, metal Q and metai J, to couple to iron nail. They prepared an agar medium with KgFe(CN); and phenolphthalein. Their professor informed them that metal Q forms an orange color while metal J forms maroon color when oxidized. Their professors also gave them the reduction half-reactions for the corresponding metal ions including the reduction of Fe 12-+ 2e -J Fe* + 2e- Fe E° =- 1.66 V E° = - 0.44 v Q2- + 2e-Q O2 + 2H20 + 4e- 40H* What color in the set-up indicates reduction process for Fe nail coupled with metal Q? E° =.0.25 v E° = + 0.40 v A pink B) orange blue maroon

A group of students were tasked to perform the metal coupling of iron nail similar to Experiment 3: Corrosion of Metals. They were given two metals, metal Q and metai J, to couple to iron nail. They prepared an agar medium with KgFe(CN); and phenolphthalein. Their professor informed them that metal Q forms an orange color while metal J forms maroon color when oxidized. Their professors also gave them the reduction half-reactions for the corresponding metal ions including the reduction of Fe 12-+ 2e -J Fe* + 2e- Fe E° =- 1.66 V E° = - 0.44 v Q2- + 2e-Q O2 + 2H20 + 4e- 40H* What color in the set-up indicates reduction process for Fe nail coupled with metal Q? E° =.0.25 v E° = + 0.40 v A pink B) orange blue maroon

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...

See similar textbooks

Similar questions

1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -0.52 V (minus 0.52 V). 2.Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.1M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.46 volts.
5
2 /2 瓦,可 106% Q 6: Galvanic cell presented as Fe/Fe² //Co²/Co, If reduction potential of iron = - 0.409 V, and for cobalt - 0.28 V, a- Calculate the electromotive force of the cell. b- Write the total reaction for the cell.
Calculate the time (minutes) required for a constant current of 0.750 A to deposit 0.270 g of cobalt (II) as cobalt (II,III) oxide [Co3O4] on the anode. Assume 100% current efficiency for both cases.
Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate symbol to separate substances in the list.) Cr³+, Ba²+, Au³+, Cu²+, K+, and Cd²+ Help chemPad XX → Greek
Use the References to access important values if needed for this question. Enter electrons as e". Use smallest possible integer coefficients. If a box is not needed, leave it blank. Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Mg metal is put into a 1M aqueous Crs+ solution. If a reaction will occur, write a balanced net ion equation for the reaction. If no reaction will occur, leave all boxes blank. + ↑
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe (aq) + H2(g) Fe(s) + 2H (aq) Hint: Carry at least 5 significant figures during intermedliate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG" for this reaction would be than zero.
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg2+(aq) + 2Cu+(aq)Hg(1) + 2Cu2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be than zero.
Write a balanced half-reaction for the oxidation of chromium ion symbols where appropriate. 00 (Cr³+) to dichromate ion (Cr₂0²-) ₁ ローロ in basic aqueous solution. Be sure to add physical state ? 000 Ar
Use the standard reduction poten Pb2(aq) + 21(aq) → Pb(s) + Hint: Carry at least 5 significant antilogarithm. You may use the C Equilibrium constant: AG° for this reaction would be
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 1₂(s) + Hg(1) 21 (aq) + Hg²+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AGº for this reaction would be greater than zero.