Consider the two reactions. 2 NH3(g) + 3N2O(g) + 4N2(g) + 3H2O(1) 4 NH3(g) + 302(g)...
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)
Consider the two reactions. 2 NH2(g) + 3 N2O(g) → 4N2(g) + 3 H2O(1) 4 NH,(g) + 30,(g) + 2 Ng(g) + 6H2O(1) AH° = -1010 kJ AH° = 1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N2(g) + 2O2(g) → N2O(g) AH° =
Consider the two reactions. 2 NH2(g) + 3 N2O(g) → 4N2(g) + 3 H2O(1) 4 NH,(g) + 30,(g) + 2 Ng(g) + 6H2O(1) AH° = -1010 kJ AH° = 1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N2(g) + 2O2(g) → N2O(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...
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
Consider the two reactions. 2 NH,(g) + 3 N, O(g) - 4N, (g) + 3H,O(1) 4NH,(g) + 30,(g) — 2N, (g) + 6H, 0(1) AH = -1010 KJ AH = 1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N,(g) + 40,(8) NO(g) AH- AHL
Hint: No calculations are required. For the reaction 2NH3(g) + 3N2O(g)— *4N2(g) + 3H2O(g) AH° = -880 kJ and AS° = 288 J/K At standard condi u conditions, this reaction would vould be product favored O at no temperature. O at all temperatures. O at relatively low temperatures. O at relatively high temperatures.
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...
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
Given the standard enthalpy changes for the following two reactions: (1) N2(g)-202(g) N204(g) ΔΗ 9.2 kJ (2) 2N2O(2N2()-O2() what is the standard enthalpy change for the reaction: (3) 2N20(D -302( 2N204() AH-? kJ