Question

Question 1

1. In the reaction: CO₂(g) + C(s) --> 2CO(g), how might the concentration of C(s) (graphite) affect the equilibrium concentration of the product CO(g)?

   	a.	It does not affect it at all because C(s) is not included in the expression of the equilibrium constant. Thus, whether C(s) is present or not does not affect the reaction.
   	b.	It doesn't affect it as long as there is C(s) present during the reaction (i.e. C(s) is in excess so it does not disappears during the reaction). In this case, the concentration of C(s) is considered constant and the equilibrium constant is calculated based only on CO2 and CO
   	c.	It can affect it if C(s) is the limiting reagent. In this case, the initial moles of CO2(g) would need to be modified to consider that the reaction can only proceed up until C(s) is consumed.
   	d.	All of the above are correct
   	e.	Only (b) and (c) are correct Question 2 The reaction: A(g) + B(g) --> 2C(g) has an equilibrium constant (Kc) of 15.51 at 700K Calculate the value of Qc if the initial concentrations of reactants and products are [A] = 0.0100 M; [B] = 0.0120 M and [C] = 0.0500 M. Use 4 significant figures in your answer Question 3 For the reaction in the question above, according to the value of Qc, in which way would the reaction proceed? a. It would proceed to the right because Qc > Kc b. It would proceed to the right because Qc < Kc c. It would proceed to the left because Qc > Kc d. It would proceed to the left because Qc < Kc e. It is already at equilibrium because Qc = Kc so the reaction will not move to the right or to the left.

Answer 1

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