Question

Calculate the ΔGr0 of the following reaction and state whether it is spontaneous at standard temperature or not. (You will need Table B-12 in your CRG.)

2HCl(aq) + Ca(OH)₂(s) CaCl₂(s) +2H₂O(1)
O 6.5 kJ, yes
O 61.5 kJ, no
O 61.5 kJ, no
O 6.5 kJ, no
O-61.5 kJ, yes
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Answer 1

Step-by-step explanation:

The ΔG° of a reaction can be calculated using the formula:

ΔG° = ΔH° - TΔS°

where ΔH° is the standard enthalpy change, ΔS° is the standard entropy change, and T is the absolute temperature in Kelvin.

From Table B-12 in the CRG, we have:

ΔH° = -65.2 kJ/mol for the reaction

ΔS° = -111.7 J/(mol*K) for the reaction

We need to convert ΔS° to kJ/(molK):

ΔS° = -111.7 J/(molK) × (1 kJ/1000 J) = -0.1117 kJ/(mol*K)

Now we can calculate ΔG°:

ΔG° = ΔH° - TΔS°

ΔG° = -65.2 kJ/mol - (298 K) × (-0.1117 kJ/(mol*K))

ΔG° = -65.2 kJ/mol + 33.4 kJ/mol

ΔG° = -31.8 kJ/mol

The negative value of ΔG° indicates that the reaction is spontaneous at standard temperature. Therefore, the answer is: 6.5 kJ, yes. However, this is not one of the options provided.