Calculate ΔG0 for each reaction using ΔGf0 values: a.)H2(g) + I2(s)  →2HI(g) b.) MnO2(s) + 2CO(g) →Mn(s) + 2CO2(g) c.)NH4Cl(s) →NH3(g) + HCl(g)

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.

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. Do not enter units with your answer N2 (g) + 3 H2 (g) → 2 NH3 (g)             ΔG° = -33.3 kJ P(N2) = 1.0 atm, P(H2) = 3.0 atm, P(NH3) = 9.0 atm

Use thermodynamic values in the table provided to calculate the ΔG for the following process in two ways.                    4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) at 25˚C   a) Use Free Energy values to calculate ΔG. b) Use Enthalpy and Entropy values with Gibbs Equation to calculate ΔG. c) What do your final ΔG values tell us about this reaction?