Write the equilibrium constant expression for the reaction 2 NO (g) + Br2 (g) ↔ 2 NOBr (g)
Do you want Kc or Kp?
Kc = (NOBr)^2/(NO)^2(Br2)
Oh, I see we're balancing equations now? Alright, let's put on our chemistry cap. The equilibrium constant expression for this reaction is Kc = [NOBr]^2 / ([NO]^2 [Br2]). But remember, even in chemistry, equilibrium is just a fancy way of saying "I don't feel like doing anything anymore." So, keep calm and let the molecules oscillate at their own pace.
The equilibrium constant expression for the reaction 2 NO (g) + Br2 (g) ↔ 2 NOBr (g) can be written as follows:
Kc = [NOBr]^2 / ([NO]^2 * [Br2])
where [NOBr], [NO], and [Br2] represent the concentrations of NOBr, NO, and Br2, respectively.
To write the equilibrium constant expression for a reaction, we use the molar concentrations of the reactants and products raised to the power of their respective stoichiometric coefficients, which represent the balanced equation.
In this reaction: 2 NO (g) + Br2 (g) ↔ 2 NOBr (g)
The equilibrium constant expression, denoted as Kc, is given by:
Kc = ([NOBr]^2) / ([NO]^2 * [Br2])
Here:
- [NOBr] represents the molar concentration of NOBr.
- [NO] represents the molar concentration of NO.
- [Br2] represents the molar concentration of Br2.
The square brackets indicate the molar concentrations, and the powers represent the stoichiometric coefficients in the balanced equation.
Please note that the equilibrium constant may vary depending on the specific temperature and pressure conditions of the reaction.