(a) If Qc>Kc how must the reaction proceed to reach equilibrium? (b) At the start of a certain r

(a) If Qc>Kc how must the reaction proceed to reach...

Key Concepts

Initial Reaction Conditions and Qc Value

At the start of a reaction where only reactants are present, the concentrations of products are zero. Since the reaction quotient is calculated using these concentrations, Qc will have an initial value of zero, indicating that the reaction will proceed in the forward direction to form products until equilibrium is achieved.

Comparison of Qc and Kc to Determine Reaction Direction

By comparing the reaction quotient (Qc) to the equilibrium constant (Kc), one can predict how the reaction will shift to reach equilibrium. If Qc is greater than Kc, the reaction will shift to the left (toward reactants) to re-establish equilibrium; if Qc is less than Kc, it will shift to the right (toward products).

Reaction Quotient (Qc)

The reaction quotient is a numerical value that expresses the ratio of the concentrations of products to reactants at any given point in a reaction, using the same form as the equilibrium constant expression. It helps in determining the direction in which a reaction will proceed to reach equilibrium.

Equilibrium Constant (Kc)

The equilibrium constant is a fixed value at a given temperature for a particular reaction, representing the ratio of the concentrations of products to reactants when the reaction is at equilibrium. It provides a benchmark for comparing the current state of the reaction with its equilibrium state.

Transcript

00:01 So in this problem we are given that with an relation between qc and kc where qc is greater than kc.

00:13 And in first part of this question, we have to find out how much the reaction will proceed to reach the equilibrium.

00:19 So the qc is the reaction quotient, which is basically so, for example, if we have a reaction like this, a plus b, produce in an equilibrium with c and d d where small ab cd are the coefficient of the reactants ab and the product cd now for this reaction the value of qc will be c over c times d over d over and then over the reactants concentrations again so this is basically also the expression for the k c at the equilibrium that means case this expression is for kc only at equilibrium but the reaction quotient is a value which which can be which can be calculated at any stage of the reaction so that doesn't matter whether the reaction is at equilibrium or not but the value of kc is exactly the value of this ratio at the equilibrium so if we have a larger value or a greater value of qc than kc that means the reaction is not at equilibrium and larger value of qc means we have a larger amount of the products present since the larger value of qc means the larger value of the numerator that means we have more products present in the reaction mixture and if we need to achieve equilibrium or if you need to reach the equilibrium that means we need to reach the value of kc and if we need to reach the value of kc we have to lower the value of kc and how we can lower that we can decrease the amount of our product and increase the amount of our reactant so by favoring the reaction or favoring the reverse reaction or just or by forming or producing some of the reactants, we can increase the value of the concentration of the reactants and we can decrease the concentration of the products.

03:08 And in this way, we can decrease the value of qc.

03:11 And at some point, we'll have the value of qc equal to kc...

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