For the reaction below, AG° = -15.0 kJ/mol at 962 K. If at 962 K, an excess of the solid A(s) is added to the gases B(g) and C(g) both having partial pressures of 0.94 atm, which statement is true? Als) 2B(g) + 2C(g) The reaction quotient will become negative. The reverse reaction will proceed spontaneously. The reaction will be at equilibrium. The equilibrium constant will increase. The forward reaction will proceed spontaneously.

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.

The equilibrium constant, Keq, for the reaction 2 HI (g) = H2 (9) + 12 (g) is 1.14 x 10-3 at 25 °C. Calculate AG* for this reaction. O 1.53 x 10-3 kJ -37.8 kJ O 6.79 kJ 16.8 kJ O-76.1 kJ

For a certain chemical reaction, the standard Gibbs free energy of reaction at 15.0 °C is 86.1 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K =0 x10 X Ś