Consider the reaction: 2A(g) + B(g) → 2C(g) If ΔG° = −−5.4 kJ/mol at T = 25°C and PA = PB = 1 atm and PC = 4 atm, which of the following statements is correct? (R = 8.314 J/K • mol) Group of answer choices Under the current conditions, ΔG > 0. Hence, this reaction will go in the forward direction to reach equilibrium. This reaction favors the products because ΔG° < 0. K < 1, because ΔG > 0. This reaction favors the reactants because ΔG° < 0.

Consider the following rection:             2 A(g) + B2(g) ⇌  2 AB(s)            ΔG° = -166.1 kJ Calculate ΔGrxn (kJ) for the reaction at 77.6 oC by using the partial pressures given below. (R=8.314 J/molK)             PB2 = 0.344 atm,  PA = 0.337 atm Report your answer with one decimal. Enter numbers only; do not enter units.

ΔG= ΔH-TΔS If ΔH=0, what does this mean regarding to the ΔS  if the ΔG for the reaction is +3.4 kJ/mol?

Consider the reaction 2NO 2( g) --> N 2O 4( g); Δ H° = –56.8 kJ and Δ S° = –175 J/K. In a container (at 298 K) N 2O 4( g) and NO 2( g) are mixed with initial partial pressures of 2.4 atm and 0.42 atm, respectively. Which of the following statements is correct?   a. Some N2O4(g) will decompose into NO2(g).   b. Some NO2(g) will dimerize to form N2O4(g).   c. The system is at equilibrium at these initial pressures.   d. The final total pressure must be known to answer this question.   e. None of these.