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Consider the following reaction at 25 °C. CO2 (g) + 2NH3 (g) → CO(NH2 )2 (s)...

Consider the following reaction at 25 °C. CO2 (g) + 2NH3 (g) → CO(NH2 )2 (s) + H2 O(l) ; ∆H° = -134kJmol-1

Which of the following is correct regarding this reaction?

(1) ∆S° is always a negative value for the reaction.

(2) ∆H° increases with the temperature.

(3) The decrease in the entropy change can determine the spontaneity of the reaction.

(4) The reaction is spontaneous at all temperatures.

(5) At high temperatures the value of ∆G° becomes more negative

Pls explain the answer?

.

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