An ionic compound readily dissolves readily in water at room temperature with an

Question

An ionic compound readily dissolves readily in water at room temperature with an enthalpy of solution 33. kj/mole. What is the sign of the Gibbs free energy for this process at room temp? (B) Does the enthalpy favor dissociation? (C) Is the entropy change positive of negative? (D) Will the dissolution become more or less favorable as the temperature increases? True or False. The reaction: COCl_2 (g) rightarrow CO (g) + Cl_2 (g) is not spontaneous at room temperature. Low temperature will favor the reaction. ___ (B) All reactions with a negative Delta G proceed quickly. ____ (C) A compound with a positive Delta G_f degree is thermodynamically unstable. ___ (D) 1 M HNO_3 (aq) will dissolve lead. ____

Explanation / Answer

A)

since ionic compound readily dissolve, the reaction must be spontaneous

So, G must be negative

B)

H is positive

we know that

G = H - T*S

Since H is trying to make G positive, enthalpy doesn’t favour dissociation

C)

G = H - T*S

Since H is positive and G is negative. So, S must be positive

Answer: positive

D)

G = H - T*S

Since S is positive, as T increases, G will become more negative and hence dissolution is more favourable

Answer: more

I am allowed to answer only 1 question at a time

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