The following substances are ordered with increasing entropy: ice < liquid water < steam.

The entropy change for the following reaction will be positive:

2SO₂ (g) + O₂ (g) → 2 SO₃ (l)

Calculate the entropy change D_freezeS^o when 1.00 mol of ethanol at its melting point (T_m = 158.8 K) freezes (in the process the temperature does not change and D_fusH^o for ethanol is + 4.64 kJ mol^-1).

Calculate the change of entropy (in J K^-1 mol^-1) when 1 mol of cyclohexane is heated at constant pressure from 20 °C to 40 °C, the molar heat capacity, C_p, of cyclohexane is 156 J K^-1 mol^-1, assume that the molar heat capacity, C_p is constant over this temperature range.

When 1 mol of a solvent is heated from 5 °C to 10 °C at constant pressure, the change of entropy is + 8.00 J K^-1 mol^-1. When the solvent is heated further from 25 °C to 30 °C, the change in entropy will also be + 8.00 J K^-1 mol^-1.

The standard entropy of methanol, at 1 bar, is 127 J K^-1 mol^-1. At 315 K, its standard entropy will be larger.

The standard entropy change for the following reaction will be large and positive: CH₃OH (g) + CO (g) à CH₃CO₂H (l)

In the organic laboratory, a procedure results in the precipitation of crystals in a conical flask. This violates the Second Law of thermodynamics.

The standard enthalpy change for the decomposition of magnesium carbonate is 100.6 kJ mol⁻¹. The standard entropy change is 174.8 J mol⁻¹ K⁻¹. Calculate the standard Gibbs energy change, DG^o (298 K), for this reaction.

Using  data given below:

Calculate the standard Gibbs energy change,  (kJ mol^-1), for the following reaction:

2SO₂ (g) + O₂ (g) → 2 SO₃ (l)

The standard enthalpy change for decomposition of CaCO₃ (s) to CaO (s) and CO­₂ (g) is 178 kJ mol⁻¹ and the standard entropy change is 161 J K⁻¹ mol⁻¹. Estimate the minimum temperature at which this reaction becomes spontaneous.