Fe3O4 +4H2 -3Fe +4H2O
?H=151 KJ and ?S=169 J/K
At what temperatures will this reaction be spontaneous?
dG° < 0, reaction becomes spontaneous.
So, dG° = dH - TdS = 151000 - T*169 < 0
On solving, we will get
T > 893.49 K
Hence at temperature greater than 893.49 K reaction will become spontaneous as dG° becomes negative.
If you have any questions please comment
If you satisfied with the solution please rate it thanks....
Fe3O4 +4H2 -3Fe +4H2O ?H=151 KJ and ?S=169 J/K At what temperatures will this reaction be...
Consider the reaction: Fe3O4(s) + 4H2(g)—>3Fe(s) + 4H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.79 moles of Fe3O4(s) react at standard conditions. ASºsystem = J/K
Consider the following reaction: Fe3O4(s) + 4H2(g) --heat--> 3Fe(s) + 4H2O(l) What mass (in g) of Fe3O4 is needed to consume 1.05 g of H2? Enter only the numeric value of your answer (no units).
Consider the following reaction: Fe3O4(s) + 4H2(g) --heat--> 3Fe(s) + 4H2O(l) What mass (in g) of Fe3O4 is needed to consume 2.17 g of H2? Enter only the numeric value of your answer (no units).
Consider the following reaction: Fe3O4(s) + 4H2(g) --heat--> 3Fe(s) + 4H2O(l) What mass (in g) of Fe3O4 is needed to consume 1.52 g of H2? Enter only the numeric value of your answer (no units).
Consider the following reaction: 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g) How many grams of steam must react to produce 370. g of Fe,O ?
1.) Consider the reaction: Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.48 moles of Fe3O4(s) react at standard conditions. G°rxn = kJ 2.)Consider the reaction: H2(g) + Cl2(g)2HCl(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.750 moles of H2(g) react at standard conditions. G°rxn = kJ
2. In a study of the reaction 3Fe (1) + 4H20) Fe3O4 (0) + 4H2O at 1200 K it was observed that when the equilibrium partial pressure of water vapor is 15.0 torr, that the total pressure at equilibrium is 36.3 torr. Calculate the value of K, for this reaction. (Hint: Apply Dalton's Law of Partial Pressures)
For a given reaction, AH is 111 kJ and AS is -249 J/K. At what temperatures is the reaction spontaneous? A. T< 446 K B. None. The reaction is never spontaneous. C. The reaction is spontaneous at all temperatures. D.T> 73 K E.T>446 K
6. What is the equilibrium constant expression for the following equilibrium? 3Fe(s) + 4H2O16) 5 Fe3O4(s) + 4H2(B) A. K = [H21 B. K = H21 [H20] C. K = [H21 [H2O]" D. K = [Fe2O3][H214 [Fe][H20]
For a particular chemical reaction Delta H =6.8 kJ and Delta S = -29 J/K. Under what temperature condition is the reaction spontaneous? A) When T < -234 K B) When T < 234 K C) The reaction is spontaneous at all temperatures D) When the reaction is not spontaneous at any temperatures E) When T > 234 K