Consider the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(1) for which AH° = -752.2 kJ and AS° = -351.6 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.549 moles of NO(g) react under standard conditions at 298.15 K. Suniverse = (2) Is this reaction reactant or product favored under standard conditions? ✪ J/K (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored choose 'reactant favored'. C

Consider the reaction 6CO2(g) + 6H20((1) C,H12O6 + 602(g) for which AH° = 2.801×10° kJ and AS° = -259.0 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.722 moles of CO2(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 reactant favored, choose 'reactant favored'.

The decomposition of copper (1) oxide to its elements does not occur spontaneously at 375°C (AG = 140.0 kJ): Cu₂0 (s) 2 Cu (s) + 1/2O₂(g). It can be made to occur spontaneously by being coupled to the oxidation of solid carbon to form carbon monoxide gas at this same temperature (AG = -143.8 kJ): C(s) + 1/2O₂(g) → CO (g) What product(s) is/are produced as a result of coupling the two reactions? CO (g) 2 Cu (s) and 1/2 O₂ (g) 2 Cu (s) and CO (g) 2 Cu (s), 1/2 O2 (g), and CO (g) 1/2 0₂ (g)

Consider the following reaction: C(graphite) + 1/2 O2 (g) → CO(g) Is it spontaneous under standard conditions at 298 K? Answer this question by calculating AS" (system), AS° (surroundings), and AS (universe). (Define reactants and products as the system.) S* (J/mol · K) A¡H° (kJ/mol) at 298 K (kJ/mol) Compound at 298 K C(s, graphite) 5.6 CO(g) 197.674 -110.525 CS2 (g) 237.8 116.7 CCL (e) 214.39 -128.4 Cl2 (g) 223.08 Si(s) 18.82 SİCL, (g) 330.86 -662.75 S(s, rhombic) 32.1 Br2 (e) 152.2 HBr(g) 198.70 -36.29 H2 (g) 130.7 H2O2 (e) 109.6 -187.78 O2 (g) 205.07 O yes O no

A reaction has AH = -112 kJ and ASan = 354 J/K. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings?

"M" represents a metallic element.  "X" represents a nonmetallic element.  Calculate ΔH for the process M3X4(s) ⟶ 3M(s) + 2X2(g) from the following information: M(s) + ½X2(g) ⟶ MX(s)  ΔH°= -286.2 kJ 3MX(s) + ½X2(g) ⟶ M3X4(s)  ΔH°= -84.3 kJ

See image for question. Please answer with units of kJ.

Determine the standard entropy of NO(g) given the following information: NO(g)+0,(g) → NO, (g) AS xn = -73.2 J/K Substance S° (J/mol · K) NO2(3) 240.0 O2(g) 205.0 NO(g) ? O -210.7 J/K O +210.7 J/K +108.2 J/K -108.2 J/K O +54.1 J/K