Under standard conditions, a given reaction is endergonic (i. e., δg > 0). which of the following can render this reaction favorable: using the product immediately in the next step, maintaining a high starting-material concentration, or keeping a high product concentration? view available hint(s) under standard conditions, a given reaction is endergonic (i. e., δg > 0). which of the following can render this reaction favorable: using the product immediately in the next step, maintaining a high starting-material concentration, or keeping a high product concentration? maintaining a high starting-material concentration keeping a high product concentration using the product immediately in the next step and maintaining a high starting-material concentration using the product immediately in the next step

Maintaining a high starting-material concentration can render this reaction favorable.

Explanation:

A reaction is favorable when ΔG < 0 (exergonic). ΔG depends on the temperature and on the reaction of reactants and products as established in the following expression:

ΔG = ΔG° + R.T.lnQ

where,

ΔG° is the standard Gibbs free energy

R is the ideal gas constant

T is the absolute temperature

Q is the reaction quotient

To make ΔG < 0 when ΔG° > 0 we need to make the term R.T.lnQ < 0. Since T is always positive we need lnQ to be negative, what happens when Q < 1. Q < 1 implies the concentration of reactants being greater than the concentration of products, that is, maintaining a high starting-material concentration will make Q < 1.

the answer is barium and copper bromide

you gotta add the following molecules so we can give u an answer

explanation: