Consider the reaction C(graphite) → C(diamond).

(a) Can graphite be converted spontaneously into diamond at T=250C and P=1atm? Explain your answer.

(b) If not, will the pressure have to be lowered or increased to achieve a spontaneous process? Explain your answer.

(c) If your answer to (b) is increased then estimate the minimum pressure necessary to allow the spontaneous reaction. Otherwise, estimate the maximum pressure at which this spontaneous reaction can take place (at T=250C).

(d) Let’s call the value of the pressure you found in Part (c) P*. In practice, do you think a spontaneous reaction can be observed at P=P* and T=250C? Explain your answer.

You can use the following information to solve this problem: The densities of graphite and diamond are 2.25 g/cm3 and 3.51 g/cm3, respectively; ΔGf(diamond)=2900J/mol

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