Take data of "Introduccion a la termodinamica en ingenieria
quimica, J.M, Smith; H. Van Ness 7° Edition":
ΔGºfH2CO(g)=-10230J/mol ΔHºGCO2(g)=-394359
ΔHºGH2O(l)=-237129J/mol;
ΔGºfO2=0
Then:
:
If 2,48 moles of H2CO react:
It need information about Phosphorus pentoxide( P4O10) acid like free energy of gibbs formations or Enthalpy formation Or entropy.
Use the References to access important values if needed for this question. Consider the reaction: Using...
Use the References to access important values if needed for this question. Consider the reaction: CH4(g) + 2O2(g) +CO2(g) + 2H2O(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.43 moles of CH4(g) react at standard conditions. AG®rx = Submit Answer Retry Entire Group 9 more group attempts remaining
Use the References to access important values if needed for this question. Consider the reaction 2CH.) + 70 (8) - 4CO2(g) + 6H2O(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.56 moles of CH @ react at standard conditions. AS surroundings J/K Submit Answer Retry Entire Group 9 more group attempts remaining
Use the References to access important values if needed for this question. Consider the reaction Fe(s) + 2 HCl(aq) FeCl2(s) + H2(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K. ANSWER:
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
Use the References to access important values if needed for this question. For the reaction 2NO(g) + O2(g) -2NO2(g) AGⓇ - 70.1 kJ and Asº -146.5J/K at 301 K and 1 atm. The maximum amount of work that could be done by this reaction when 2.00 moles of No(@react at standard conditions at this temperature is kJ.
References) Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Zn2+(aq) + Ni(s)— Zn(s) + Ni2+(aq) Answer: kJ K for this reaction would be than one. Submit Answer Retry Entire Group 4 more group attempts remaining
[References) Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Ca2+(aq) + Zn(s) Cl(s) + Zn2+ (aq) Answer: kJ K for this reaction would be than one. Submit Answer Retry Entire Group 4 more group attempts remaining
please help Use the References to access important values if needed for this question. For the reaction 2NO(g) + O2(g)—2NO2(g) AGⓇ --63.8 kJ and AS - -146.5 J/K at 344 K and I atm. The maximum amount of work that could be done by this reaction when 1.76 moles of NO(g) react at standard conditions at this temperature is kJ. Submit Answer Retry Entire Group 9 more group attempts remaining lo access important values if needed for this question. For...
reg References Use the References to access important values if needed for this question. For the reaction NH,NO3(aq) N2O(g) + 2 H2O(1) AGⓇ --181.6 kJ and AH° -149.6 kJ at 320 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 320 K. The entropy change for the reaction of 2.46 moles of NH NO3(aq) at this temperature would be J/K. Submit Answer
Consider the reaction: Fe(s) + 2HCl(aq) +FcC12(8) + H2(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.46 moles of Fe(s) react at standard conditions, AG xn Submit Answer Retry Entire Group 8 more group attempts remaining Consider the reaction: N2(g) + O2(g) +2NO(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.690 moles of N.() react at standard conditions. kJ AG Submit Answer Retry Entire Group & more group attempts remaining