Question

From the thermodynamic data, ΔSsys for the given fuel cell reaction is negative but the reaction...

From the thermodynamic data, ΔSsys for the given fuel cell reaction is negative but the reaction is still spontaneous. How can the negative entropy of the system be justified as spontaneous or is it simply violation of second law of thermodynamics? Explain in detail the various factors that can lead to the spontaneity of this reaction. ½ O2(g) + H2(g) → H2O(l)

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider a hydrogen-oxygen fuel cell, an electrochemical cell that generates electricity from the chemical reaction 2...
Consider a hydrogen-oxygen fuel cell, an electrochemical cell that generates electricity from the chemical reaction 2 H2(g) + O2(g) → 2 H2O(l) . Yes, this is the same reaction as in additional question 1, but now we are looking at electrochemical aspects of it. On one side of the cell, H2 is pumped in, and the half-cell reaction is 2 H2(g) + 4 OH–(aq) → 4 H2O(l) + 4 e– ; at the other side, O2 is pumped in: O2(g)...
Consider a fuel cell that uses the reaction of ethanol with oxygen to produce electricity, CH3CH2OH...
Consider a fuel cell that uses the reaction of ethanol with oxygen to produce electricity, CH3CH2OH (l) + 3O2 (g) -----> 2CO2 (g) + 3 H2O (l) Use thermodynamic data (https://sites.google.com/site/chempendix/thermo) to determine the value of E°cell for this cell at 25 °C.
Consider the reaction: 2H2O(l)2H2(g) + O2(g) Using standard thermodynamic data at 298K, calculate the entropy change...
Consider the reaction: 2H2O(l)2H2(g) + O2(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.88 moles of H2O(l) react at standard conditions. S°surroundings = J/K
Hydrogen is oxidized in a fuel cell to make electricity, by the (unbalanced) reaction: H2 +...
Hydrogen is oxidized in a fuel cell to make electricity, by the (unbalanced) reaction: H2 + O2  H2O. 1 kg/min H2 is fed to the fuel cell, and oxygen is fed as 21% of air. The oxygen is fed at a rate 50% more than the minimum required to completely oxidize all the H2. Assuming that all the Hydrogen is consumed, find the molar flow rate of all chemical species leaving the fuel cell.
To study a key fuel-cell reaction, a chemical engineer has 20.0−L tanks of H2 and of...
To study a key fuel-cell reaction, a chemical engineer has 20.0−L tanks of H2 and of O2 and wants to use up both tanks to form 26.0 mol of water at 23.8°C. (a) Use the ideal gas law to find the pressure needed in each tank. ___ atm H2 ____ atm O2 B. Use the van der Waals equation to find the pressure needed in each tank. ____ atm H2 ____atm O2
1) For which of the following processes does entropy decrease? A. H2(g) + Cl2(g)   →   2HCl(g)...
1) For which of the following processes does entropy decrease? A. H2(g) + Cl2(g)   →   2HCl(g) B. N2(g) + 3H2(g)   → 2NH3(g) C. Making amorphous glass from crystalline SiO2 (quartz) D. CH3OH(l) → CH3OH(aq) 2) Use the values provided in the table to calculate the standard free energy change for the following reaction at 298 K:   2H2O2(g)  → 2H2O(g) + O2(g)   Substance ∆Gf° (kJ/mol) at 298 K H2O(g) −228 H2O2(g) −105 A −666 kJ B +666 kJ C +246 kJ D −246...
Burning H2 (g) in the presence of O2 (g) proceeds by the following reaction:                         H2...
Burning H2 (g) in the presence of O2 (g) proceeds by the following reaction:                         H2 (g) + ½ O2 (g) --> H2O (g)                       eq. 1 In a fuel cell, the oxidation half-reaction occurring at the anode (a solid conductor) is: H2 (g) --> 2H+ (aq) + 2e- eq. 2 At the cathode (solid conductor), O2 is reduced: O2 (g) + 4H+ (aq) + 4e- --> 2H2O (l) eq. 3 Using Hess’s Law, estimate the heat released by oxidizing...
Shown below are the reactions occurring in the direct methanol fuel cell (DMFC). I 2 CH3OH(aq)...
Shown below are the reactions occurring in the direct methanol fuel cell (DMFC). I 2 CH3OH(aq) + 2 H2O(l) → 2 CO2(g) +12 H+(aq) +12 e- II 3 O2(g) + 12 H+(aq) + 12 e- → 6 H2O(l) Overall 2 CH3OH(aq) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) Which is the anode reaction, and what is being oxidized in the overall reaction? II, O2 I, H2O II, H+ IV, CH3OH
1) Given the following thermochemical reaction and thermodynamic data, find Gibbs Free Energy, ΔG, and determine...
1) Given the following thermochemical reaction and thermodynamic data, find Gibbs Free Energy, ΔG, and determine if the reaction is spontaneous or non-spontaneous at 25 °C? N2(g) + 3H2(g) → 2NH3(g) ΔH = -91.8 kJ ΔS[N2] = 191 J / mol · K, ΔS[H2] = 131 J / mol · K, and ΔS[NH3] = 193 J / mol · K a.98.3 kJ; Non-Spontaneous b.-98.3 kJ; Spontaneous c.32.7 kJ; Non-Spontaneous d.ΔG = -32.7 kJ; Spontaneous 2) What is the oxidation number...
1- Calculate ΔG o for the following reaction at 25°C. You will have to look up...
1- Calculate ΔG o for the following reaction at 25°C. You will have to look up the thermodynamic data. 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) 2- A reaction will be spontaneous only at low temperatures if both ΔH and ΔS are negative. For a reaction in which ΔH = −320.1 kJ/mol and ΔS = −99.00 J/K ·mol,determine the temperature (in °C)below which the reaction is spontaneous.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT