The statements in the tables below are about two different chemical equilibria.

Question

The statements in the tables below are about two different chemical equilibria. The symbols have their usual meaning, for example

K stands for the equilibrium constant.

The statements in the tables below are about two different chemical equilibria. The symbols have their usual meaning, for example Go stands for the standard Gibbs free energy of reaction and K stands for the equilibrium constant. In each table, there may be one statement that is false because it contradicts the other three statements. If you find a false statement, check the box next to it. Otherwise, check the "no false statements" box under the table. statement false? statement false? In K>0 no false statements: no false statements:

Explanation / Answer

if

dS° > dH°/T

dS°T > dH

0 > dH -dS°T

dG = dH -dS°T then

dG > 0, this must be false, since

dG <0, which states K > 1, thereofre, ln(K) > 0

choose A as incorrect.

Q2

dS° = dH°/T

dH° - T*dS° = 0

dG = 0, this is in equilbirium

so

K = 1, in equilbirium correct,

ln(K) = ln(1) = 0

then

dG° = 1, is false, dG° can have many other values

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