The spontaneity of a reaction can be determined using the Gibbs Free Energy equation, which is ΔG = ΔH - TΔS.

In this case, ΔH (change in enthalpy) is 620 kJ/mol and ΔS (change in entropy) is -0.46 kJ/(molK).

For a reaction to be spontaneous, ΔG must be less than 0.

Let's calculate the temperature at which ΔG = 0, because above this temperature, the reaction will be spontaneous.

0 = 620 kJ/mol - T * -0.46 kJ/(molK)

Rearranging the equation gives:

T = 620 kJ/mol / 0.46 kJ/(molK) = 1347.83 K

Therefore, the reaction is spontaneous above 1347.83 K.

So, the correct answer is A. It is spontaneous above 1347 K.

Question

The spontaneity of a reaction can be determined using the Gibbs Free Energy equation, which is ΔG = ΔH - TΔS.

In this case, ΔH (change in enthalpy) is 620 kJ/mol and ΔS (change in entropy) is -0.46 kJ/(molK).

For a reaction to be spontaneous, ΔG must be less than 0.

Let's calculate the temperature at which ΔG = 0, because above this temperature, the reaction will be spontaneous.

0 = 620 kJ/mol - T * -0.46 kJ/(molK)

Rearranging the equation gives:

T = 620 kJ/mol / 0.46 kJ/(molK) = 1347.83 K

Therefore, the reaction is spontaneous above 1347.83 K.

So, the correct answer is A. It is spontaneous above 1347 K.

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