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)?

The decomposition of ammonia is: 2NH3(g) -> N2(g) + 3H2(g). If the pressure of ammonia is 1.0 × 10^-3 atm, and the pressures of N2 and H2 are each 0.20 atm, what is the value of Kp' at 400°C for the reverse reaction?

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

In a solution at equilibrium with both PbSO4 and SrSO4, what is the relationship between the concentrations of [SO4^2-], [Pb^2+], and [Sr^2+]?

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−?