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Which of the following statements is correct concerning thevalue of the equilibrium constant of the reaction below?PbO(s) + CO(g) Pb(l)+ CO2(g)Group of answer choi...

Question

Which of the following statements is correct concerning thevalue of the equilibrium constant of the reaction below?PbO(s) + CO(g) Pb(l)+ CO2(g)Group of answer choicesKc = When carbon dioxide gas is removed, the value ofKc will decrease.The greater the value of Kc, the higher is the ratioof inthe equilibrium mixture.For the given reaction, Kc KP.The greater the value of Kc, the faster the reactionwill reach equilibrium.

Which of the following statements is correct concerning the value of the equilibrium constant of the reaction below? PbO(s) + CO(g) Pb(l) + CO2(g) Group of answer choices Kc = When carbon dioxide gas is removed, the value of Kc will decrease. The greater the value of Kc, the higher is the ratio of in the equilibrium mixture. For the given reaction, Kc KP. The greater the value of Kc, the faster the reaction will reach equilibrium.



Answers

Which of the following statements is true regarding the general equilibrium expression? (a) $K_{\text {eq }}$ for gaseous equilibria does not depend on temperature. (b) $K_{\text {eq }}$ for gaseous equilibria does not include solid substances.

They, um a plus B unequal. Every must see. And this is Cave one, and we're starting to see to a plus to be goes to four c. So the coefficients have doubled, which means that K two is equal to K one squared because doubling the coefficients would raise the equilibrium constant to the power to, So this would be option beans.

In this problem were given two different statements regarding a chemical reaction system in equilibrium, and we need to determine which one of these is true. We think about a system in equilibrium of reacting a reverse oblique producing product. Be. We know that we conform equilibrium, constant expression for Casey to be the concentration of B divided by the concentration of a In both of those are the equilibrium concentrations of each one of those species. And the first statement, part A says the concentrations of reactant and products are equal. Well, that could be the case, but it is not necessarily true. Whatever the equilibrium concentrations are when we divide them, they have to come out to this value of K C at a certain temperature. So that is not a true statement all the time. However, statement B is correct. The rate of the forward and reverse reactions are equal. That is the definition of any system and in chemical system at equilibrium. So that is why B is the correct answer in this case. So again it does not. Equilibrium does not mean that the concentrations of the reactions and products are equal, even though for a system in equilibrium that could be the case. Whatever the equilibrium, concentrations are at a certain temperature. The ratio those concentrations defines the equilibrium constant at that temperature and at equilibrium, the rates of the forward and reverse reactions are equal. That is how we define dynamic equilibrium in the system because reactant sin products are still forming. But their rates at which there forming or equal. So that is why statement B is.

The value of K is defined as the concentration of the products divided by the concentration of the reactions. Now I feel a bit specific here. It's the concentration of all the products in equilibrium, divided by the concentration of all the reactant said equilibrium. So for a, um, the initial concentration of the reactant so okay does not depend on the initial concentration of reactions. It's the equilibrium concentration that matters for B. The initial concentration of products okay, does not depend initial concentration of products for C the temperature of the system que does depend on the temperature of system, whether endo thermic for excellent. But we need to know that information pad for D The nature of the reactant que does depend on the nature of reactant and we can go further here. Solids are not included. Pure liquids are not included. Onley gas fees and Equus phase are included, so those air the ones that are included so it does depend on the nature of the reactions

This question has a Siris of conceptual statements regarding the equilibrium constant. It states that the equilibrium, constant value is dependent upon the initial concentrations of the reactant, the initial concentrations of the products, the temperature or the nature of the reactant and the products. The only two statements that are valid are the last two C and D, the temperature of the system and the nature of the reactant and the products, the initial concentrations and the initial. The initial concentrations of the reactant and products do not alter the K value at all. The K value stays constant and is used to determine the final concentrations of the reactant and products. However, the equilibrium constant does change as a function of temperature. According to the vaunt Hoff equation, the vault Hoff equation shows that the natural log of the K value is a function of one over the kelvin temperature. The K value is also dependent upon the nature of the reactant and the products. If they are solids or pure liquids, they're not part of the equilibrium. Constant expression and their concentrations do not affect the K value at equilibrium. For example, in these two chemical reactions water is a gas where it is part of the equilibrium, constant expression and can change the K value where at, for the second reaction at equilibrium, the product of water is a liquid and is not part of the equilibrium, constant expression. So these two reactions, where the nature of the product is different would have two different equilibrium, constant values.


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