At 25 ∘C, the equilibrium partial pressures for the reaction   A(g)+2B(g)↽−−⇀C(g)+D(g) were found to be ?A=5.01 atm, ?B=4.25 atm, ?C=5.14 atm, and ?D=5.75 atm. What is the standard change in Gibbs free energy of this reaction at 25 ∘C?

Consider the following equilibrium: +N2g3H2g    2NH3g =       ΔG0−34.kJ Now suppose a reaction vessel is filled with  2.58atm  of nitrogen  N2  and  3.27atm  of ammonia  NH3  at  647.°C . Answer the following questions about this system: Under these conditions, will the pressure of  NH3  tend to rise or fall?   rise     fall   Is it possible to reverse this tendency by adding  H2 ?In other words, if you said the pressure of  NH3  will tend to rise, can that be changed to a tendency to fall by adding  H2 ? Similarly, if you said the pressure of  NH3  will tend to fall, can that be changed to a tendency to rise by adding  H2 ?   yes     no   If you said the tendency can be reversed in the second question, calculate the minimum pressure of  H2  needed to reverse it.Round your answer to  2  significant digits. atm

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H6(g)+H2(g)↽−−⇀2CH4(g) the standard change in Gibbs free energy is  Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are  ?C2H6=0.250 atm ,  ?H2=0.200 atm , and  ?CH4=0.850 atm ?

Decreasing the temperature of the reaction CO (g) + ½ 02 → CO2 (g) favors (A) (B) Products Reactants