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...
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)
Homework Answers
If the reaction is reversed then the value of ∆H° is doesn't change the sign of the value is reversed.
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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...
Consider the two reactions. 2 NH3(g) + 3N2O(g) + 4N2(g) + 3H2O(1) 4 NH3(g) + 302(g)...
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. 2 NH2(g) + 3 N2O(g) → 4N2(g) + 3 H2O(1) 4 NH,(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)...
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° =
Calculate standard free energy change using AGvalues. Consider the reaction 2NH3(g) + 3N2O(g)—>4N2(g) + 3H2O(g) Use...
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 reaction 2NH3(g) + 3N2O(g) 4N2(e) + 3H2O(g) for which AH = -879.5 kJ and...
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...
Predict the sign and calculate ASⓇ for a reaction. Consider the reaction 2NH3(g) + 3N2O(g) +4N2(g)...
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...
(ii) Calculate AH° for the reaction N2H4(1) + O2(g) → N2(g) + 2H2O(1) using the data...
(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
Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2NH3(g) + 2O2(g)N2O(g) + 3H2O(l) kJ
Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2NH3(g) + 2O2(g)N2O(g) + 3H2O(l) kJ
Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(...
Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ 2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ H2O(l)→H2O(g), ΔH∘D=+44 kJ
6. Consider the following equilibrium, 2N2(g) + 6H20(0) 4NH3(g) + 3O2(g) AH =-1531 kJ/mol a. Write...
6. Consider the following equilibrium, 2N2(g) + 6H20(0) 4NH3(g) + 3O2(g) AH =-1531 kJ/mol a. Write the equilibrium constant expression for K. and for Kp, if appropriate, for the reaction. b. State whether the equilibrium is heterogeneous or homogeneous. c. State how the equilibrium would respond to the addition of some of the water from the system. d. State how the equilibrium would respond to a decrease in the partial pressure of ammonia (NHa). e. State how the equilibrium would...
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. 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° =
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 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...
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...
(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
6. Consider the following equilibrium, 2N2(g) + 6H20(0) 4NH3(g) + 3O2(g) AH =-1531 kJ/mol a. Write the equilibrium constant expression for K. and for Kp, if appropriate, for the reaction. b. State whether the equilibrium is heterogeneous or homogeneous. c. State how the equilibrium would respond to the addition of some of the water from the system. d. State how the equilibrium would respond to a decrease in the partial pressure of ammonia (NHa). e. State how the equilibrium would...
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