Answer those blank. Show complete solutions. (c) Consider the equation for hydrogen consumption mµ2 in a fuel cell:P,(W)H, usage(kg/s) =1.05×10*V (V)Convert this equation to one where hydrogen usage is reported in mol/hr.Jason M. KeithStudent ViewSupplemental Material for Elementary Principles of Chemical ProcessesStrategyWe can use unit conversions to determine a new equation for the hydrogen consumptionrate.SolutionStart with the equation and the given units, writing the usage rate as a ratio of mass perunit time.Mass (kg)H, usage(kg/s) =Time (s)Then we have:2.02(g) (kg)Mass (kg) = Moles (mol)-Moles(mol) 1000(g)And we also have:60 (s)Time (s) = Minutes(min).= 60Minutes(min)Substituting into the left hand side of the formula for hydrogen usage, we have:Mass (kg)MolesMolesH¸ usage(kg/s) =Time (s)60MinutesMinutesInserting into the full formula for hydrogen usage, we have:P,(W)H, usage(mol/min) =V,(V)

Given, H2 usage (kg/s) = Mass (kg) / Time (s) Time (s) = Minutes (min) * 60 (s) / (min) = 60…

Answered: Mass (kg) H, usage(kg/s) = Time (s)…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 83QRT

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Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
lus engine.html?ClassID=1246112631# ent Orie... Using the data from the previous steps, calculate the standard Gibbs Free Energy for the formation of rust at 25°C. 2Fe(s) + 3H2O(g) → Fe2O3(s) + 3H2(g) ASn = -117 J/K AHn = -140 kJ rxn %3D rxn AGn = [ ?] kJ Enter either a + or - sign AND the magnitude. Free Energy (kJ) Enter
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