Using the S° of formation of the standard states of its elements, identify the ΔS° for the formation of POCl₃(g).  

Decarboxylation reactions are those in which a carboxyl group is removed and releases CO₂. The following reaction shows the decarboxylation of malonic acid:

(CH₂(COOH)₂)(s) → CH₃COOH(l) + CO₂(g)

Assume that ΔH° and ΔS° do not vary with temperature, determine the minimum temperature at which this reaction will occur spontaneously under standard conditions. 

                                         ΔH° (kJ/mol)          S° (J/mol•K)
(CH₂(COOH)₂)(s)              –891.1                     149.0
CH₃COOH(l)                    –487.0                    159.8
CO₂(g)                             –393.5                    213.6

Using the following reactions with known ΔG°_rxn values:

H₂(g) + 1/2 O₂(g) → H₂O(g)         ΔG°_rxn = –228.6 kJ
3 O₂(g) → 2 O₃(g)                       ΔG°_rxn = 326.4 kJ

Calculate the ΔG° for the following reaction:

3 H₂(g) + O₃(g) → 3 H₂O(g)        ΔG°_rxn = ?

At 25°C, what are the ΔS°_rxn, ΔH°_rxn , and ΔG°_rxn for the following reaction? 

Is the reaction spontaneous? If not, will changing the temperature make it spontaneous? If so, should it be increased or decreased?

The following figures illustrate the initial state and equilibrium state of the reaction X₂(g) ⇌ 2 X(g). 

Determine whether the reaction is spontaneous or nonspontaneous. What are the signs (+, −, or 0) of ΔH, ΔS, and ΔG when the reaction proceeds from its initial state to the equilibrium state?

Which one of these statements about ∆G and ∆G° is correct?

A) Q > 1: ΔG < ΔG° because RTlnQ is negative 

B) Q = 1: ΔG = ΔG° because RTlnQ is 0

C) Q < 1: ΔG > ΔG° because RTlnQ is positive

What happens to the thermodynamic tendency for the reaction to take place, when the value of Q decreases?

In the diagram below, the yellow line represents ΔH while the blue line represents TΔS. The diagram illustrates the change of ΔH and TΔS with temperature for a theoretical reaction:

Identify the range of temperatures where the reaction occurs spontaneously.

The reaction SO₂ (g) + 1/2 O₂ (g) ⇌ SO₃ is involved in the production of acid rain. The standard free energy of each substance is given below. 

ΔG°_f, SO2(g) = −300.1 kJ/mol

ΔG°_{f, O2 (g)} = 0

ΔG°_{f, SO3(g)} = −371.1 kJ/mol

What is the equilibrium pressure of SO₂ in the system at 298 K when P_SO2 = P_O2 and P_SO2 = 45 torr?

Using the following data, 

ΔG°_f NaHSO₄(s) = −992.8 kJ/mol

ΔG°_f NaOH(s) = −379.7 kJ/mol

ΔG°_f SO₃(g) = −371.1 kJ/mol

What is the K_c expression for the reaction? What are the K_c value and ΔG° value for the reaction at 298 K?

NaHSO₄(s) ⇌ NaOH(s) + SO₃(g)

For the reaction A(aq) ⇌ 2 B(aq) + C(aq), K_c = 124.6 at 30 ºC. Calculate ΔG_rxn at 30 ºC when [A] = 0.32 M, [B] = 0.25 M, and [C] = 0.18 M.