6:00 PM Fri Oct 8* 43%AAwww-awn.aleks.comG periodic table -..Favorites - YouT...TV fuboTVALEKS - Caliyah...Watch...G kno3 acid or ba...G linear program...G write formulas f...Solved A. Chem...O CHEMICAL REACTIONSPredicting whether simple electrochemical reactions happenCaliyah vDecide whether a chemical reaction happens in either of the following situations. If a reaction does happen, write the chemical equation for it. Be sure yourchemical equation is balanced and has physical state symbols.chemicalsituationchemical equationreaction?A strip of solid lead metalis put into a beaker of0.022M AGNO3 solution.yesalonoArA strip of solid silvermetal is put into a beakerof 0.040M Pb(NO3)2O yesO nosolution.

Answered: Image /qna-images/answer/2fe3c989-59f6-40f2-82e4-f7e7cfb0244c.jpg

Answered: Decide whether a chemical reaction…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.107QE

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Similar questions

9.69 How are the roles of transmission substations and distribution substations in the electrical grid similar? How are they different?
What are the advantages of glass electrode over hydrogen electrode? Please explain briefly.
A thin circular-disk earring 4.00 cm in diameter is platedwith a coating of gold 0.25 mm thick from an Au³⁺ bath.(a) How many days does it take to deposit the gold on one sideof one earring if the current is 0.013 A (d of gold =19.3 g/cm³)?(b) How many days does it take to deposit the gold on both sidesof the pair of earrings?(c) If the price of gold is $320 per troy ounce (31.10 g), what is the total cost of the gold plating?
Initial mass of copper electrode (g) 1.201g Final mass of copper electrode (g) 1.163g Initial mass of key (g) 8.464g Final mass of key (g) 8.525g Average current (A) 0.015 A Time of current application (s) 30 min Use your current vs. time data to calculate the theoretical number of moles of copper that should have plated out onto the brass key.
How much time in minutes would it take to deposit 1.05 grams of X (MW = 64.75 g/mol) on a cathode in by a current of 3.7 A? X2+ + 2e- → X(s) Round your answer to the ones place
Initial mass of copper electrode (g) 1.201g Final mass of copper electrode (g) 1.163g Initial mass of key (g) 8.464g Final mass of key (g) 8.525g Average current (A) 0.015 A Time of current application (s) 30 min Use your data from measuring the mass of the electrode and the key to calculate the actual number of moles of copper that plated out.
I- All anodic reactions on the metal surface being protected completely stop.Il- The direction of the current in the electrolyte is from the anode to the cathode.Ill- The current intensity passing through thecircuit depends on the potential difference between the anode andcathode andtheresistanceof the circuit.IV- The surface of the metal structure to be protected cathodically can be covered with a suitable material and thecurrent requirement can be reduced. Which of the above / which are wrong?
The electrolysis of 0.500 L of molten ZnCl2 will take place. Determine the current (amperes) needed for the complete transformation of zinc if we can let the reaction proceed for 24h. The density of ZnCl2 is 2.91 g/mL.
An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a current of 9.00 A. If inert electrodes are used in the process, how many grams of copper were removed from the solution?
2. The production of hydrogen gas was made at a pressure of 15 psi from the electrolysis of water. The total volume of hydrogen gas produced is 0.004 cubic meter. Electrolysis of water takes place where a current passes through a 7.14 ohm resistor with a voltage of 25 volts for 1.5hrs. Determine the following: a. number of moles of H2 gas b. Temperature condition of the process in °C c. Energy consumed to produce H2 gas.
Which of the following statements accurately describes the Nernst equation shown below? Ecell=Ecello−nFRTlnQ
An electric current of 1.5 mA does 0.25 J of work in 1.00 min. How much voltage is driving the electrons?

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