A voltaic cell is made by placing a zinc electrode in a compartment in which the Zn2+ concentration is 2.0 × 10-5 M and by placing a Pt electrode in the other compartment,in which the H+ concentration is 3.4 M and PH2 = 1.00 atm.The Zn2+/Zn half-cell reduction potential is -0.76 V,and the H+/H2 half-cell reduction potential is 0.00 V.What is the equilibrium constant at 25°C for the spontaneous cell reaction?
A) 4 × 104
B) 5 × 1020
C) 5 × 1022
D) 7 × 10 12
E) 5 × 10 25
Correct Answer:
Verified
Q69: Given: Q70: Which of the following statements is true Q71: What is the equilibrium constant (K)at 25°C Q72: For a certain reaction,ΔHº = -75.4kJ and Q73: A voltaic cell is made by placing Q75: Which of the following statements is true Q76: For a reaction in a voltaic cell,both Q77: If E°cell for a certain reaction is Q78: If the value of E°cell is 2.10 Q79: What is E of the following cell
Unlock this Answer For Free Now!
View this answer and more for free by performing one of the following actions
Scan the QR code to install the App and get 2 free unlocks
Unlock quizzes for free by uploading documents