Which of these would most likely be one of the final steps when performing a strong acid-base titration? prepare the burette. record the initial burette volume. prepare to measure ph change. observe any changes as base is added.
here, we have to get the effect of temperature, the reaction which is exothermic.
as the temperature increase the concentration of n₂o₄ will decrease and the formation of product will be favorable.
the left to right reaction is exothermic.
the reaction is n₂o₄⇄2no₂.
now the reaction from left to right has the heat of reaction 14 kcal. thus this reaction is exothermic.
as per thermodynamics δg = δh - tδs (where, δg = gibbs free energy, δh = heat of the reaction, δs = entropy and t = temperature).
for the favorable reaction δg must be negative. thus the reaction from left to right will be favorable. also as the temperature increase the rate of the reaction from left to right will increase.