3. Use the AH° and AS° values below to determine the range of temperatures (in kelvin, K) for which the respective reaction will be favorable AH° = -904 kJ AS° = +0.179 kJ/K AH° = +173 kJ AS° = +0.176 kJ/K AH° = -139 kJ AS° = -0.286 kJ/K AH° = +285 kJ AS° = -0.138 kJ/K

What is AH° for the following reaction? 2C,H>(g) + 50,(g) → 4CO2(g) + 2H20(1) Substance AH®, (kJ/mol) C¿H>(g) +226.7 CO2(g) -393.5 H;0(!) -285.8 +2599.0 kJ -1692.2 kJ -452.6 kJ O -2599.0 kJ +1692.2 kJ

For the reactionI2(g) + Cl2(g)  2 ICl(g)G° = -30.7 kJ and S° = 11.4 J/K at 338 K and 1 atm.This reaction is (reactant, product) _______ favored under standard conditions at 338 K.The standard enthalpy change for the reaction of 2.05 moles of I2(g) at this temperature would be  ______ kJ.

For a particular reaction at 140.6 °C, AG = 560.53 kJ/mol, and AS = 131.79 J/(mol · K). Calculate AG for this reaction at -68.1 °C. AG = 467.18 kJ/mol Incorrect

Hydrogen sulfide decomposes according to the following reaction: 2H2S(g) → 2H2(g) + S2(g) - = For this reaction at 298 K, AS rxn = 78.1 J/K mol, Arxn = 169.4 kJ/mol, and AG rxn 146.1 kJ/mol. What is AG rxn at 900. K?

For the reaction 4HCI(g) + O2(g) 2H20(g) + 2C12(g) AH° = -114.4 kJ and AS° = -128.9 J/K The equilibrium constant for this reaction at 310.0 K is Assume that AH° and AS° are independent of temperature.

For a particular reaction at 128.2 °C, AG = 190.07 kJ/mol, and A.S = 658.97 J/(mol K). Calculate AG for this reaction at 21.3 °C. kJ/mol AG =

A Mo another question will save this response. stion 16 Consider the following reaction at 25°C if PpcIs=0.0029 atm, PpCi3 =0.27 atm, and PC12= 0.40 atm PC13 (0 + Cl2 (g)- PCl, (g) AH°, = -0.1702 kJ/K What is the value of O? 0.02685 What is the value of AG? -37.2KJ Is the reaction spontaneous under these conditions? Yes, the reaction is spontaner

A certain reaction has ∆?°= -19.5KJ and ∆S°= 42.7 J/K, is the reaction exothermic or endothermic?

Consider the following reaction at 25 °C: 3 Ni(s) + N2(g) + 3 H20(g) → 3 NiO(s) + 2 NH3(g) Given the information in the table, calculate AH° for the reaction.