According to relation,
Reaction is spontaneous whenever change in Gibbs free energy is negative.
For the the given reaction,
Negative,
Positive,
Hence from above data we can anticipate that for any value of temperature, Negative(always) hence reaction is spontaneous at all temperatures. Choice B is correct.
Hint: No calculations are required. For the reaction 2NH3(g) + 3N2O(g)— *4N2(g) + 3H2O(g) AH° =...
Consider the reaction 2NH3(g) + 3N2O(g) 4N2(e) + 3H2O(g) for which AH = -879.5 kJ and AS - 288.1 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.197 moles of NH3(g) react under standard conditions at 298.15 K. Asuniverse J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is...
Hint: No calculations are required. For the reaction 2BrF3(g)— Br2(g) + 3F2(g) AH° = 542 kJ and AS° = 269 J/K At standard conditions, this reaction would be product favored O at relatively low temperatures. O at no temperature. O at all temperatures. O at relatively high temperatures.
Calculate standard free energy change using AGvalues. Consider the reaction 2NH3(g) + 3N2O(g)—>4N2(g) + 3H2O(g) Use standard free energies of formation to calculate the standard free energy change for this reaction at 25°C. AG° kJ/mol
3N2O(g) + 2NH3(8) – 4N2(ə) + 3H203) AH = -879.6 kJ What is AH' for N2O in kJ.mol-1? Heats of Formation NH3 H20 - 45.9 kJ.mol-1 - 241.8 kJ-mol-1 +82 -82 -246 +246
Predict the sign and calculate ASⓇ for a reaction. Consider the reaction 2NH3(g) + 3N2O(g) +4N2(g) + 3H2O(g) Based upon the stoichiometry of the reaction the sign of ASørxn should be ' Using standard thermodynamic data (in the Chemistry References), calculate A Sºrxn at 25°C. AS rx = J/Komol Consider the reaction 4NH3(g) + 502(g) +4NO(g) + 6H2O(g) where AS rx = 180.5 J/K Using standard thermodynamic data in the Chemistry References), calculate the entropy change of the surroundings and...
Consider the two reactions. 2 NH3(g) + 3N2O(g) + 4N2(g) + 3H2O(1) 4 NH3(g) + 302(g) + 2N2(g) + 6H2O(1) AH° = -1010 kJ AH° = 1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N,(8) + O2(8) + N20(8) AH° = k.
Consider the two reactions. 2NH3(g)+3N2O(g)4NH3(g)+3O2(g)⟶4N2(g)+3H2O(l)⟶2N2(g)+6H2O(l) Δ?∘=−1010 kJΔ?∘=1531 kJ2NH3(g)+3N2O(g)⟶4N2(g)+3H2O(l) ΔH∘=−1010 kJ4NH3(g)+3O2(g)⟶2N2(g)+6H2O(l) ΔH∘=1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N2(g)+12O2(g)⟶N2O(g)N2(g)+12O2(g)⟶N2O(g)
please help with those 3 questions thank you so much Review Topic [References Use the References to access important values if needed for this question. M Hint: No calculations are required. M For the reaction Bred 2CO() + 2NO(g)2CO2(g) + N2(2) 8 AH° = -747 kJ and AS = -198 J/K M At standard conditions, this reaction would be product favored at relatively high temperatures. at no temperature. os Зreg O at all temperatures. O at relatively low temperatures. 3reg...
please help with these Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.37 moles of Fe2O3() react at standard conditions. AS system JK 2CO(g) + O2(g) +2CO2(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.54 moles of CO(g) react at standard conditions. AS system JK 2NH3(g) + 3N20(g)— 4N2(g) + 3H2O(g) AH = -879.5 kJ and AS° = 288.1 J/K The...
(ii) Calculate AH° for the reaction N2H4(1) + O2(g) → N2(g) + 2H2O(1) using the data given below: 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(1) N2O(g) + 3H2(g) → N2H4(l) + H2O(1) 2NH3(g) + O2(g) → N2H4(1) + H2O(1) H2(g) + 1/2O2(g) → H2O(1) AH° = -1010. kJ AH° = -317 kJ AH° = -143 kJ AH° = -286 kJ