Kc Calculation for BrF5 ↔ Br2 + 5F2 Reaction

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In summary, the Kc calculation for the reaction between BrF5 and Br2 + 5F2 involves determining the equilibrium constant using the concentrations of the reactants and products at equilibrium. This calculation can be used to predict the direction of the reaction and the relative amounts of reactants and products present at equilibrium. The Kc value can also be affected by changes in temperature, pressure, or the addition of a catalyst. Overall, the Kc calculation is a useful tool in understanding the behavior of the BrF5 ↔ Br2 + 5F2 reaction.
  • #1
Mag
2BrF5 ↔ Br2 + 5F2
If we wanted to solve for Kc (Kc=product/reactants) would we assume that the products are on the right side of the equation. In other words would we set it up like this

[BrF5]^2 / [Br2] [F2]^5 or


[Br2][F2]^5 / [BrF5]^2
 
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  • #2
The latter. Yes, by convention, the RHS contains the products.

By this convention, LHS -> RHS is considered the forward direction/reaction and RHS -> LHS is considered the reverse reaction.
 
  • #3
assuming that the latter corresponds to the rate limiting reaction...yes.


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FAQ: Kc Calculation for BrF5 ↔ Br2 + 5F2 Reaction

What is the equation for the reaction between BrF5 and Br2?

The equation is BrF5 ↔ Br2 + 5F2, which shows the reversible reaction between BrF5 and its products, Br2 and 5F2.

How do I calculate the equilibrium constant (Kc) for this reaction?

The equilibrium constant (Kc) can be calculated by taking the concentration of the products, Br2 and F2, and dividing it by the concentration of the reactant, BrF5. This equation can be written as Kc = [Br2][F2]^5/[BrF5].

What is the significance of the equilibrium constant (Kc) for this reaction?

The equilibrium constant (Kc) is a measure of the extent to which the reaction proceeds towards the products. A high Kc value indicates that the reaction favors the formation of products, while a low Kc value indicates that the reaction favors the reactant.

Can the equilibrium constant (Kc) change with temperature?

Yes, the equilibrium constant (Kc) is affected by changes in temperature. An increase in temperature can shift the equilibrium towards the products, resulting in a higher Kc value. Conversely, a decrease in temperature can shift the equilibrium towards the reactant, resulting in a lower Kc value.

How does the stoichiometry of the reaction affect the equilibrium constant (Kc)?

The stoichiometry of the reaction, specifically the coefficients of the reactants and products, directly affects the equilibrium constant (Kc). In this reaction, the coefficient of BrF5 is 1, while the coefficients of Br2 and F2 are 1 and 5, respectively. This means that for every 1 mole of BrF5 that reacts, 1 mole of Br2 and 5 moles of F2 are produced. Therefore, the equilibrium constant (Kc) is calculated based on the concentration of the products raised to their respective coefficients, while the concentration of the reactant remains unchanged.

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