What can be said about an endothermic reaction with a negative entropy change? spontaneous at all temperatures. spontaneous at high temperatures. spontaneous at low temperatures. spontaneous in the reverse direction at all temperatures. nonspontaneous in either direction at all temperatures. submit

spontaneous in the reverse direction at all temperatures

Explanation:

The parameter to predict the spontaneity of a reduction is the change in the free energy, ΔG.

This is how it works:

If ΔG = 0, the system is in equilibriumIf ΔG > 0, the reaction is non-spontaneous.If ΔG < 0, the reaction is spontaneous.

In brief, free energy's decrease tells that a reaction is spontaneous, while free energy's increase tells a reaction is nonspontaneous.

Now, take the definition of the free energy:

G = H - TSΔG = ΔH - TΔS

The conditions given in the statement are:

An endothermic reaction ⇒ ΔH > 0 (positive)A negative entropy change ⇒ ΔS < 0 ⇒ TΔS < 0 (negative)

Replacing in the equation ΔG = ΔH - TΔS, you get:

ΔG = positive - (negative) = positive + positive = positive.

Then, you conclude that for an endothermic reaction with a negative entropy change, the change in the free energy is positive, and so the reaction is nonspontaneous (at all temperatures) in the forward direction.

Since, the change in the reverse direction has opposite sign, you also conclude that the reaction is spontaneous in the reverse direction at all temperatures.

If the water vapor content stays the same and the temperature drops, then the relative humidity increases. its vise versa.if the water vapor content stats the same and the temperature rises, the relative humidity decreases. so, yes, i'd say that temperature and humidity have a strong relationship.

10.063g / 10.00 ml = 1.0063 g/ml which rounds off to 4 sig figs as: 1.006 g/ml