For an endothermic reaction, how will the value for Keq change when the temperature is increased?
2 answers:
Answer:
C. Keq will increase
Explanation:
Endothermic means the reaction will <em>absorb heat</em> to occur, hence an increase in temperature will favor the reaction, increasing the formation of products.
Keq is the equilibrium constant of the reaction, and it can be defined as:
In an endothermic reaction the equilibrium will be shift towards the formation of products when the temperature is increased, the concentration of products will increase (in relation to the concentration of reactants) ; so as a result the equilibrium constant Keq will also increase.
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Answer:
0.758 V.
Explanation:
Hello!
In this case, case when we include the effect of concentration on an electrochemical cell, we need to consider the Nerst equation at 25 °C:
Whereas n stands for the number of moles of transferred electrons and Q the reaction quotient relating the concentration of the oxidized species over the concentration of the reduced species. In such a way, we can write the undergoing half-reactions in the cell, considering the iron's one is reversed because it has the most positive standard potential so it tends to reduction:
It means that the concentration of the oxidized species is 0.002 M (that of nickel), that of the reduced species is 0.40 M and there are two moles of transferred electrons; therefore, the generated potential turns out:
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