Trevor dissolves sodium hydroxide pellets in a beaker of water at room temperature, and notes that the beaker becomes warm. which correctly designates the signs of δh, δs, and δg for this process?

a. δh > 0, δs > 0, and δg < 0
b. δh < 0, δs > 0, and δg < 0
c. δh > 0, δs > 0, and δg > 0
d. δh < 0, δs < 0, and δg > 0

B. ΔH < 0, ΔS > 0, and ΔG < 0

Explanation:

As the beaker gets warm ,the energy has been released when Trevor dissolves sodium hydroxide pellets in a beaker of water. Thus as the energy has been released in the reaction, the reaction is exothermic and the change in enthalpy i.e. is negative and is less than zero.

The entropy is the measure of degree of randomness. The entropy increases when the randomness increases and the entropy decreases when the randomness decreases. When a substance dissolves in water, it dissociate into ions and hence the randomness increases thus the change in entropy i.e.  is positive and  is more than zero.

also

That is change in gibbs free energy i.e. is negative and is less than zero.

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