For a galvanic cell under standard conditions based on the reaction below,the zinc is increasing in mass.Zn(s) + 2Ag*(aq) → Zn2*(aq) + 2Ag(s) E°cell 1.56 VYou AnsweredTrueCorrect AnswerO FalseQuestion 7If AG for a reaction is greater than zero, thenYou Answeredmore information is needed.Correct AnswerK<1please explain why this is wrong and what theanswer should be

For given reaction, the E°cell is positive and therefore the reaction is going in forward direction.…

For a galvanic cell under standard conditions based on the reaction below, the zinc is increasing in mass. Zn(s) + 2Ag (aq) → Zn2*(aq) + 2Ag(s) E°cell 1.56 V You Answered True Correct Answer False Question 7 If AG° for a reaction is greater than zero, then K 1 You Answered more information is needed. Correct Answer K<1 X-0

For a galvanic cell under standard conditions based on the reaction below, the zinc is increasing in mass. Zn(s) + 2Ag (aq) → Zn2*(aq) + 2Ag(s) E°cell 1.56 V You Answered True Correct Answer False Question 7 If AG° for a reaction is greater than zero, then K 1 You Answered more information is needed. Correct Answer K<1 X-0

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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Q10
Give the standard line notation for each cell below (Pt electrode both cathode and anode) a. Cr3+(aq) + Cl2(g) ⟶ Cr2O72- (aq) + Cl-(aq) b. Cu2+(aq) + Mg(s) ⟶ Cu(s) + Mg2+(aq)
A concentration cell running at 25°C consists of two Al(s)/Al3+(aq) cells. If the concentration of Al3+ at the anode is 4.12 x 10-8 M and the concentration of Al3+ at the cathode is 1.27 M, what is the value of Ecell? (Two decimal places)
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MISSED THIS? Read Section 20.5 (Pages 913 - 917) ; Watch KCV 20.5. Calculate AG°n and Ecell at 25° C for a redox reaction with n = 4 that has an equilibrium constant of K = 4.8x10-2. Part A Express your answer using two significant figures. AG° rxn = kJ Submit Request Answer Part B Express your answer using two significant figures. να ΑΣφ E cell = Submit Request Answer Provide Feedback
Consider an electrolytic cell with a steady current of 169 amperes which produces Al(s) (atomic mass = 26.98 g/mol) according to the equation below. 2A1,0 31) + 3C (s) -4AI +3CO (s) 2(g) What is the time, in hours, needed to produce 218 g of Al(s)? Show your answers in two decimal places. Do NOT include units in your final answer.
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