The equilibrium constant for the reaction 2NO(g) + Br2 ⇌ 2NOBr(g) is Kc = 2.0 × 10⁻² at a certain temperature. Calculate Kc for the reverse reaction NOBr(g) ⇌ NO(g) + 1/2Br2(g).

Given the equilibrium constant for the reaction H2(g) + Br2(g) ⇌ 2 HBr(g) is Kc = 3.8 × 10^4, what is the equilibrium constant for the reverse reaction 4 HBr(g) ⇌ 2 H2(g) + 2 Br2(g)?

Given the following reactions and their equilibrium constants, calculate the equilibrium constant (Kc) for the reaction: 2A(g) + B(g) ⇌ A2B(g). Reaction 1: A2B(g) + B(g) ⇌ A2B2(g), Kc = 16.4 Reaction 2: 2A(g) + 2B(g) ⇌ A2B2(g), Kc = 28.2

Given the reaction 2COF2(g) ⇌ CO2(g) + CF4(g) with an equilibrium constant Kp = 2.2 × 10^6 at 298 K, what is the equilibrium constant Kp for the reaction 4COF2(g) ⇌ 2CO2(g) + 2CF4(g)?

What is the concentration of aqueous CO2 in the reaction CO2(g) ⇌ CO2(aq) with a Kc of 0.83, given the partial pressure of CO2(g) is 2.53 atm?

Given the equilibrium reaction CO2(g) ⇌ CO2(aq) with an equilibrium constant Kc of 0.83, what is the concentration of aqueous CO2 if the concentration of gaseous CO2 is 1.0 M?

What is the equilibrium constant expression for the reaction Fe(OH)3(s) + C2O42− ⇌ [Fe(C2O4)3]3−(aq) + OH−?

Which of the following expressions represents the equilibrium constant (K) for the dissolution of urea in water, given the mass of urea and the initial and final temperatures?