There are two stable states of CaCO3 known as Aragonite and Calcite. Using infor

Question

There are two stable states of CaCO3 known as Aragonite and Calcite. Using information from the table reference data at the back of the book. A) Which form is the stable state at 298 K and 1 bar. B) Calculate the pressure where the second state states becomes stable and C) Calculate the temperature at which the second state becomes stable. For simplicity you may assume that both the change in S and the change in V are zero over these temperature and pressure ranges.

Here is the information from the back of the book.

          deltaH(kJ), deltaG(kJ), S(J/K), Cp(J/K), V (cm^3)

Calcite -1206.9, -1128.8, 92.9, 81.88, 36.93

Aragonite -1207.1, -1127.8, 88.7, 81.25, 34.15

I have done the problem but I'm not 100% sure its right.

Explanation / Answer

a)

  calcite is more stable as its delta G or gibbs free energy is more negative than that of aragonite.

also calcite S(entropy) is more positive than that of aragonites.

also heat of formation is also more.

b)

delta G = delta H - T*(delta S).

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