Under standard conditions (250 C, 1.0 atm): i. If Cr metal is immersed in a solution of Zn(NO3)2, will the Cr metal be/can be oxidized? ii. Calculate the standard cell potential (in V) at 250C for a Galvanic cell prepared with a Cr electrode in a Ca(NO3)3 solution and a Zn electrode in a Zn(NO3)2 solution. iii. Write the reaction and the cell notation

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Chapter18: Electrochemistry
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Problem 9RQ: What characterizes an electrolytic cell? What is an ampere? When the current applied to an...
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Cr(s)
salt bridge
-Zn(s)
2.50 M
0.20 M
Zn(NO3)2
Cr(NO3)3
Cr³+ (aq) + 3e →Cr (s)
Eºred= - 0,740 V
Zn²+ (aq) + 2e → Zn (s)
Eºred= - 0,763 V
R = 8,314 J mol-¹ K-1 dan = 9,650* 104 J/Volt mol e
Under standard conditions (250 C, 1.0 atm):
i. If Cr metal is immersed in a solution of Zn(NO3)2, will the Cr metal be/can be oxidized?
ii. Calculate the standard cell potential (in V) at 250C for a Galvanic cell prepared with a Cr electrode in a Cr(NO3)3
solution and a Zn electrode in a Zn(NO3)2 solution.
iii. Write the reaction and the cell notation
jv. Calculate the equilibrium constant
Transcribed Image Text:Cr(s) salt bridge -Zn(s) 2.50 M 0.20 M Zn(NO3)2 Cr(NO3)3 Cr³+ (aq) + 3e →Cr (s) Eºred= - 0,740 V Zn²+ (aq) + 2e → Zn (s) Eºred= - 0,763 V R = 8,314 J mol-¹ K-1 dan = 9,650* 104 J/Volt mol e Under standard conditions (250 C, 1.0 atm): i. If Cr metal is immersed in a solution of Zn(NO3)2, will the Cr metal be/can be oxidized? ii. Calculate the standard cell potential (in V) at 250C for a Galvanic cell prepared with a Cr electrode in a Cr(NO3)3 solution and a Zn electrode in a Zn(NO3)2 solution. iii. Write the reaction and the cell notation jv. Calculate the equilibrium constant
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