6 (13 pts) Given the system: 4NH3(g) + 302(g) = 2N2(g) + 6H2O(1) AH=-1530.4 kJ a) Discuss and provide reasoning) how the ammonia (NH3) concentration will be affected at equilibrium: i) Removing 02: ii) Adding additional water: iii) Increasing volume:
Given the system: 4NH3(g) + 302(g) = 2N2(g) + 6H2O(1) AH=-1530.4 kJ a) Discuss (and provide reasoning) how the ammonia (NH3) concentration will be affected at equilibrium: i) Removing O2: ii) Adding additional water: iii) Increasing volume:
Confused on #5
5) Calculate the enthalpy of the following reaction: N2 + O2 ---> 2NO Given: 4NH3 + 502 ---> 4NO + 6H2O AH° = -1170 kJ 2N2 + 6H2O ---> 4NH3 + 302 AH° = +1530 kJ Solution:
Review Problem 6.088 Given the following thermochemical equations, 4NH3(g) +70,(3) — GNO (8) + 8NH3(g) — 4NO2(g) + 6H20(3) AH°=-1132 kJ N(8) + 12H,0(8) AH = -2740 kJ calculate the value of AH (in kilojoules) for the reaction 4NH3(g) + 30,($) — 2N,() + 6H20(g) AH The number of significant digits is set to 4; the tolerance is +/-2% Show Work is REQUIRED for this question: Open Show Work
Review Problem 6.086 Given the following thermochemical equations, 2Cu + S(s) - Cu2S(s) AH° = -79.5 kJ S(s) + O2(g) → SO2(9) AH = -297 kJ Cu2S(s) + 202(g) → 2CụO(s) + SO2(g) AH° = -527.5 kJ calculate the standard enthalpy of formation (in kilojoules per mole) of Cuo(s). AH°(Cuo(s)) - kJ/mol The number of significant digits is set to 3; the tolerance is +/-2% Show Work is REQUIRED for this question: Open Show Work Review Problem 6.087 Given the...
From the following equations, calculate AH for the reaction 2N2(g) + + 5O2(g) → 2N2O5(g) AH = ? H2(g) + O2(9) H206) AH = -285.8 kJ N2O5(g) + H200 2HNO30 AH = -76.6 kJ N2(g) + 302(g) + H219) - 2HNO30) AH = -348.2 kJ
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)
Question 20 (3 points) Given the following reactions N2 (g) + 202(g) → 2N02 (8) AH = 66.4 kJ 2NO(g) + O2(g) → 2N02 (8) AH =-114.2 kJ the enthalpy of the reaction of the nitrogen to produce nitric oxide N2 (8) + O2(g) → 2NO(g) is __________ kJ. O 47.8 O-180.6 0-47.8 O 180.6 90.3
A chemist measures the enthalpy change AH during the following reaction: 3 N2(9) + 8H2(9)→ 4NH3(g) + N,H.(1) AH=-134. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH NH,() +,() - N,(6) + H_() X 5 ? 4NH, (g) + N,H.(1) 3N, (g) + 8H,() k 3 z N. (8) + 4H, (p) + 44,() + 2NH3(g) + ŹN,H,()
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...