Chemical Thermodynamics_II

Calculate the ΔH˚ for the following reaction (in kJ/mol):

Ag⁺ (aq) + Cl^- (aq) ⇌ AgCl (s)

     Substance

ΔH_f˚(kJ/mol)

Ag⁺ (aq) = 105.90

Cl^- (aq) = -167.2

AgCl (s) = -127.0

• +65.7

• -55.7

• 75.7

• -65.7

Tags

NGSS.HS-PS1-4

Calculate the ΔS˚ for the following reaction (in J/mol-K):

Ag⁺ (aq) + Cl^- (aq) ⇌ AgCl (s)

     Substance

S˚(J/mol•K)

Ag⁺ (aq) = 73.93

Cl^- (aq) = 56.5

AgCl (s) = 96.11

• -23.3

• -34.3

• +34.3

• -43.4

What is the ΔG˚ for a reaction (in kJ/mol) if ΔH˚ = -65.7 kJ/mol and ΔS˚ = -34.32 J/mol.K?

• -55.5

• +55.5

• 25.5

• -555

• The reaction is spontaneous at all temperatures.

• The reaction is spontaneous at low temperatures.

• The reaction is spontaneous at high temperatures.

• The reaction is non-spontaneous at all temperatures.

Tags

NGSS.HS-PS1-4

• positive

• negative

• zero

• none of the above

• All of the above statements are correct.

Which of the following statements is incorrect?

Tags

NGSS.HS-PS3-4