A solution is prepared by dissolving solid ammonium nitrate, NH4NO3, in water. The initial temperature of the water was 25oC, but after the solid had dissolved, the temperature had fallen to 20oC. What conclusion may be made about delta H and delta S

ΔH is positive, ΔS is positive

Explanation:

The enthalpy of reaction (ΔH) is positive in an endothermic reaction. An endothermic reaction leads to a decrease in temperature. Hence the fact that the temperature was decreased from 25oC to 20oC shows that the reaction is endothermic therefore ΔH is positive.

Also, the equation of the dissolution is;

NH4NO3(s) > NH4^+(aq) + NO3^-(aq)

This means that the number of particles in solution were increased. The entropy increases with increase in number of particles hence ΔS is positive.

it should be all of them because it asks if you included all of those in your answer

explanation:

the answer for sodium is 0.186

the answer for rubidium is 0.251