Entropy & Spontaneity (HL IB Chemistry)

This question looks at how the entropy change of water varies with temperature.

Standard entropies can be used to calculate the entropy change of a reaction, ΔS.
For example, for the formation of nitrogen monoxide from nitrogen and oxygen. 

NO (g) + O₃ (g) → NO₂ (g) + O₂ (g)

Use the data given to calculate the entropy change of the reaction between nitric oxide and ozone at 298K.

The contact process is a method used industrially to form sulfur trioxide, by reacting sulfur dioxide and oxygen together over a vanadium(V) oxide catalyst.

The equation for this reaction is shown below:

2SO₂ (g) + O₂ (g) ⇌ 2SO₃ (g)

The value for the free energy change is an indication whether the forward or backwardreaction is favoured.

The curve that we would expect to see for the reaction between sulfur dioxide and oxygen is shown below.

 Explain why the curve for this reaction is shifted to the right hand side.

The enthalpy of solution of sodium chloride is +4 kJ mol^-1. Explain why the free energy change for dissolving sodium chloride in water is negative, despite the enthalpy change being a positive value.

Calcium carbonate thermally decomposes to form calcium oxide and carbon dioxide, as shown below:

CaCO₃ (s) → CaO (s) + CO₂ (g)

The enthalpy change of the above reaction is ΔH^Θ = +178 kJ mol^-1and the entropy change is ΔS^Θ = +161 J K^-1 mol^-1 

Calculate the temperature at which the free-energy change, ΔG^Θ, for this process is zero. 

Some ionic compounds such as potassium chloride, KCl, will dissolve in water at room temperature in an endothermic process. 

KCl (s) → K⁺ (aq) + Cl^- (aq)                ΔH = +16 kJ mol^-1

Diamond and graphite are both allotropes of carbon.

Ethanol is used in large quantities in the production of alcoholic beverages and as a fuel.

The combustion of ethanol is represented by the equation:

CH₃CH₂OH (l) + 3O₂ (g) → 2CO₂ (g) + 3H₂O (g) 

The standard entropy, S^Θ, of O₂ (g) is 205 J K^-1 mol^-1.

Using the data given and Section 13 in the Data Booklet, determine the entropy change, ΔS^Θ, for the combustion of ethanol at 298K. 

Using the enthalpy of combustion for ethanol from Section 14 in the Data Booklet and the ΔS^ϴ determined in part (a), calculate the standard free energy for the combustion of ethanol.

Explain whether changing the temperature for the combustion of ethanol will alter the spontaneity of the reaction. 

Using Section 13 of the Data Booklet, explain the difference in the standard entropy values between methanol, CH₃OH and ethanol, CH₃CH₂OH. 

Ammonia, NH₃, is produced by the Haber process and is an important chemical in the manufacture of fertilisers and clearing products. 

Ammonia gas can react with oxygen to produce nitrogen monoxide and steam, and is the first step in the Ostwald process which produces nitric acid. 

Explain why the standard entropy change for the reaction is positive.

The second step in the Ostwald process produces nitrogen dioxide as shown in the equation 

2NO (g) + O₂ (g) → 2NO₂ (g)             ΔH^ϴ = -112 kJ mol^-1   

The standard entropy for NO₂ (g) is 240.0 J K^-1 mol^-1

Determine the value for the free energy change for this reaction at 298 K using the information given

Explain whether changing the temperature for the production of nitrogen dioxide will alter the spontaneity of the reaction 

The boiling point of a liquid is the temperature at which its solid and liquid phases are in equilibrium as shown in the equation for the vaporisation of water. 

            H₂O (l) → H₂O (g) 

Use Section 13 of the Data Booklet to determine values for the enthalpy change, ΔH^ϴ, and entropy change, ΔS^ϴ, for the reaction at 298 K. 

Use your answer to part (a) to estimate a temperature, in K, that the reaction becomes feasible.

Explain how your answer to part (b) could be made more accurate. 

Explain why the reaction is spontaneous above the boiling point of water.

The equations for two separate reversible reactions are as follows:

• Reaction A 2SO₂ (g) + O₂ (g) ⇌ 2SO₃ (g)
• Reaction B CO (g) + H₂O (g) ⇌ CO₂ (g) + H₂ (g)
  

Use the information in the following table to determine the enthalpy change, ΔH_r, for reaction A. 

Use your answer to parts a) and b) to determine the temperature at which reaction A becomes feasible. 

By using the data from part a) and section 13 of the data booklet, deduce if reaction B is feasible at a low temperature.

Magnesium carbonate decomposes at a relatively high temperature. 

Using your answer to part a) to determine if the decomposition of magnesium carbonate is feasible at 280 ℃. 

Using your answer to part b) to determine the temperature, in ℃, at which the decomposition of magnesium carbonate becomes feasible.

Used in the production of polymers, methanol is manufactured in large quantities.

Use section 13 of the data booklet to determine the enthalpy change, ΔH_r , for the production of methanol from carbon monoxide and hydrogen. 

A student states that if the temperature is lowered for the formation of methanol, the reaction will become non-spontaneous. Comment on the student’s statement.

The Ostwald process to produce nitric acid involves the oxidation of ammonia. The equation is shown below:

4NH₃ (g) + 5O₂ (g) → 4NO (g) + 6H₂O (g)    ΔH_r = -905.2 kJ mol^-1

The free energy change, ΔG^Θ , for the oxidation of ammonia at 298 K is -959 kJ mol^-1.
Use section 13 of the data booklet, to calculate the entropy change for the oxidation of ammonia in J K^-1 mol^-1.

Use your answer to part a) and section 13 of the data booklet to determine the standard entropy of nitric oxide gas. 

A 1.00 mol sample of NOCl was placed in reactor and heated to 227°C until the system reached equilibrium. The value for the equilibrium constant at this temperature is K_c is 4.5 x 10^-4 mol dm^-3.  

2NOCl (g)  2NO (g) + Cl₂ (g)

Write an expression for K_c. 

Using section 1 and 2 in the data booklet determine the value for the free energy change, ΔG^Θ , in kJ mol^-1 for the reaction in part c).