Corrosion of iron in water is given by, Fe + 2H+ → Fe +² + H₂(g) Calculate equilibrium constant at 298 K Calculate pH2 when pH = 10 and [Fe+²] = 10-³ M. Keq Keq = 7.49x10^14; PH2 = 0.00749 atm 468 T Keq = 3.64x10^13; PH2 = 0.0036 atm | Keq = 2.49x10^14; PH2 = 0.0749 atm FEL 7.69×10^12; PH2 = 0.0065 atm O Ke
Corrosion of iron in water is given by, Fe + 2H+ → Fe +² + H₂(g) Calculate equilibrium constant at 298 K Calculate pH2 when pH = 10 and [Fe+²] = 10-³ M. Keq Keq = 7.49x10^14; PH2 = 0.00749 atm 468 T Keq = 3.64x10^13; PH2 = 0.0036 atm | Keq = 2.49x10^14; PH2 = 0.0749 atm FEL 7.69×10^12; PH2 = 0.0065 atm O Ke
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 38P
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Question
![Corrosion of iron in water is given by,
Fe + 2H+ Fe +2 + H₂(g)
→
Calculate equilibrium constant at 298 K
Calculate pH2 when pH = 10 and [Fe2] = 10-³M.
2.5
Keq = 7.49x10^14; PH2 = 0.00749 atm
O Keq = 3.64x10^13; PH2 = 0.0036 atm
25-
Keq = 2.49x10^14; PH2 = 0.0749 atm
O Ke-7.69×10^12; PH2 = 0.0065 atm
FIL](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcbe77726-4f7a-4564-b32f-a95ee2e97d41%2F5d70de85-f592-4542-8756-67084798362c%2Fpfdyph9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Corrosion of iron in water is given by,
Fe + 2H+ Fe +2 + H₂(g)
→
Calculate equilibrium constant at 298 K
Calculate pH2 when pH = 10 and [Fe2] = 10-³M.
2.5
Keq = 7.49x10^14; PH2 = 0.00749 atm
O Keq = 3.64x10^13; PH2 = 0.0036 atm
25-
Keq = 2.49x10^14; PH2 = 0.0749 atm
O Ke-7.69×10^12; PH2 = 0.0065 atm
FIL
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