In the simulation provided, click on the Experiment menu and then click on the Run Experiment button that appears. Run each electrolysis experiment with the settings described below to complete the following paragraphs. Fillin the blanks as you proceed through each reaction or write down your results as you go to avoid having to rerun the experiments numerous times. When moving from one experiment to the next, click on the blue circular Resetbutton to reset the entire experiment or the blue circular Rerun button to reset only the settings of the ammeter (current and time).Match the words and numbers to the appropriate blanks in the sentences below. Make certain each sentence is complete before submitting your answer.• View Available Hint(s)Reset Help1 to 1Electrolysis experiment A is run to completion with the following parameters: The positiveterminal is made of Zn, the negative terminal is made of Zn, the solution is Zn(NO3)2, the11.95 gcurrent is set to 12.00 A, and the time is set to 8 min. The final mass of the positive terminal is0.49 gand the final mass of the negative terminal isThus, the total10.49 gmass of Zn metal that is electroplated is9.51 g2. Electrolysis experiment B is run to completion with the following parameters: The positivemade of Zn, the negative terminal is made of Zn, the solution is Zn(NO3)2, the3 to 1terminal1.95 gcurrent is set to 3.00 A, and the time is set to 8 min. The final mass of the positive terminal is,and the final mass of the negative terminal isThus, the totalstoichiometry with respect toelectronsmass of Zn that is electroplated iscurrent3. The ratio change in mass between experiments A and B is equal to. This8.05 gcorresponds to an identical ratio between the two experiments' values for4 to 12 to 1

As per the guideline, since you have asked multiple questions, we have solved the first question for…

Electrolysis experiment A is run to completion with the following parameters: The positive erminal is made of Zn, the negative terminal is made of Zn, the solution is Zn(NO3)2, the urrent is set to 12.00 A, and the time is set to 8 min. The final mass of the positive terminal is , and the final mass of the negative terminal is . Thus, the total nass of Zn metal that is electroplated is

Electrolysis experiment A is run to completion with the following parameters: The positive erminal is made of Zn, the negative terminal is made of Zn, the solution is Zn(NO3)2, the urrent is set to 12.00 A, and the time is set to 8 min. The final mass of the positive terminal is , and the final mass of the negative terminal is . Thus, the total nass of Zn metal that is electroplated is

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

Bookmarks Window Help www-awu.aleks.com Disney+ | Video Player O ELECTROCHEMISTRY Calculating standard reaction free energy from standard... Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction f Round your answer to 4 significant digits. 2+ 5 Zn (s) + 2103 (aq) + 12H* (aq) → 5Zn²+ (aq) + 1₂ (s) + 6H₂O (1) 2 kJ x10 Explanation dit View History ||| 200 Check JUN 9 X S C. 2. NAINE
Please answer and explain process in details.
pls.ans.wer... ASAP. I really need help. you dont have to show all the steps but just help pls. I will highly consider thumps up
A cvg.cengagenow.com eneral... Netflix Flipgrid | 50ffc... Content GRLContent Netflix Favorites My Home [Review Topics] [References] Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg** concentration is 4.25×10-4 M and the Al3+ concentration is 1.06 M ? 3Hg²"(aq) + 2AI(s)3Hg(1) + 2AI³*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Solve it asap... Standard potential can be found in Google or any book
|The electrolysis of Bio* produces pure bismuth. How long would it take to produce 7.50 g Bi by the electrolysis of a Bio* solution using a current of 27.5 A? Time min =
Use the Standard Reduction Table to answer the following questions. Write a balanced net redox equation and determine both the standard cell potential and the number of electrons transferred for the spontaneous redox process that occurs when the following couples are connected. Use the lowest possib matter under the given conditions in your answer. For the reaction arrow, please use an extensive arrow to the right (-->). d) Fe2+/Fe + Zn²+/Zn chemPad XX→← Zn (s) + Fe2+ (aq) → Zn²+ (aq) + Fe ( Zn (s) + Fe^2+ (aq) --> Zn^2+ (aq) + Fe (s) Correct. E° = .31 Reduction half-reactions Li¹+ (aq) + e¹- K¹+ (aq)+ e¹- Ba²+ (aq) + 2 e¹- Ca²+ (aq) + 2 e¹- Na¹ + (aq) + e¹- Mg²+ (aq) + 2 e¹- Al³+ (aq) + 3 e¹- U³+ (aq) + 3 e¹- Ti²+ (aq) + 2 e¹- Mn²+ (aq) + 2 e¹- 2 H₂O +2 e¹- Zn²+ (aq) + 2 e¹- Cr³+ (aq) + 3 e¹- HCHO(aq) + 2 H₂O +2e¹- Fe²+ (aq) + 2 e¹- 2 H₂O +2 e¹- X V Cd²+ (aq) + 2 e¹- PbSO4(s) + 2 e¹- In³+ (aq) + 3 e¹- Co²+ (aq) + 2 e¹- → Help Greek n (moles of e") = 2 E°(V) -3.04 -2.92 -2.92 -2.84…
1. TABLE COMPLETION. Directions: Using the following electrochemical equations, fill in the table completely and correcting. Reactions: (1) KCIO3 + C12H22O11 - KCI + H2O + CO2 Oxidizing Reducing No. Agent Agent Oxidation Reduction (1)
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 (9) == Cr2O,²- (ag) + Cl¯(aq) E = V b. Cu?+ (ag) + Ba(s) Ba²+ (ag) + Cu(s) V
Predict the products at the anode and the cathode obtained from electrolysis of a 1 M Znl2 solution. Note that 2 H20(1) + 2e → H2(g) + 2 OH(aq) E°red = -0.83 V O2(g) + 4 H*(aq) + 4e¯ → 2 H20(1) I2(s) + 2e → 2 I'(aq) Zn2*(aq) + 2e* → Zn(s) E°re = +1.23 V red E°red = +0.54 V E°, -0.76 V red = (Show work for full or partial credit.) The product at the anode is 12(s). The product at the cathode is Zn(s). The product at the anode is O2(g) and H*(aq). The product at the cathode is Zn(s). None of these The product at the anode is Zn(s). The product at the cathode is O2lg) and H*(aq). The product at the anode is O2lg) and H*(aq). The products at the cathode are H2(g) and OH (aq). The products at the anode are H2(g) and OH"(aq). The product at the cathode is O2(g) and H*(aq). The product at the anode is Zn(s). The product at the cathode is I2(s).