For a particular reaction at 212.7 °C, ΔG=−843.71 kJ, and ΔS=603.37 J/K. Calculate ΔG for this reaction at −12.4 °C.

For a particular reaction at 127.9 °C, AG = –342.08 kJ, and AS : 324.01 J/K. Calculate AG for this reaction at –73.0 °C.

Calculate the entropy change when water freezes. Standard state entropy values for water:     H2O (s)     ΔS° = 41 J·mol-1·K-1      H2O (l)     ΔS° = 70 J·mol-1·K-1      H2O (g)     ΔS° = 189 J·mol-1·K-1

A reaction is studied at various temperatures, and a graph of ln K ( equilibrium constants on y axis) versus 1/T (Temperature on x axis) is prepared in Excel. The equation of the line is found to be y = - 9500 x + 21.5.  What is the ΔSfor this reaction in J/mol/K?  (assume R=8.314Jmol⋅K)

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.

ΔG∘ for the isomerization reaction glucose-1-phosphate (G1P)⟶⟶glucose-6-phosphate (G6P) is -7.1 kJ x mol^-1. Calculate the equilibrium ratio of [G1P] to [G6P] at 25 degrees Celsius.

A certain reaction is spontaneous at 65 ° C. If the enthalpy change for the reaction is  15 kJ/mol,  what is the minimum value of  Δ S (in J/K · mol) for the reaction.

Calculate ΔG for the following reaction at 3000 K and 3.29 x 10-3 atm of Cl2(g).2AgCl(s) → 2Ag(s) + Cl2(g)       ΔG° = 220 kJInsert your answer rounded to 3 decimal digits.

Use the thermodynamic data provided below to determine the ΔGº for the reaction. 1A(s) + 4B(g) -> 1C(s) + 2D(g) Given the following: ΔGf° = -96.0 kJ mol-1 for substance A (s) ΔGfº = 254.0 kJ mol-1 for substance B (g) ΔGfº = 59.0 kJ mol-1 for substance C (s) ΔGfº= 248.0 kJ mol-1 for substance D (g) Provide your answer with final units of kJ and to one decimal place.

Calculate the standard free energy for the reaction given.  2 CH 3OH( l) + 3 O 2( g) → 2 CO 2( g) + 4 H 2O( l)     a -797.8 kJ   b -2069.8 kJ   c -1404.8 kJ   d -465.2 kJ