For a particular reaction, Δ H ∘ = 20.1 kJ/mol and Δ S ∘ = 45.9 J / (mol ⋅ K). Assuming these values change very little with temperature,
at what temperature does the reaction change from nonspontaneous to spontaneous in the forward direction? T = K

438 K

Explanation:

According to Gibbs equation:

= Gibb's free energy change

= enthalpy change = 20.1 kJ/mol = 20100 J/mol

T = temperature

= entropy change = 45.9 J/Kmol

A reaction is at equilibrium when = Gibb's free energy change is zero and becomes spontaneous when = Gibb's free energy change is negative.

T=437.9K

Thus the temperature at which the reaction change from nonspontaneous to spontaneous in the forward direction is 438 K

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.

um i think it might be a car?