Hydrogen peroxide decomposes according to the equation 2H2O2(l) → 2H2O(l) + O2(g). Calculate Kp for this reaction at 25°C given ΔH° = -98.2 kJ/mol and ΔS° = 70.1 J/K·mol.

For the reaction CO (g) + Cl2 (g) ⇌ COCl2 (g) with Kc = 255 at 1000 K, a reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.175 M at 1000 K. What is the equilibrium concentration of COCl2?

For the reaction CO (g) + Cl2 (g) ⇌ COCl2 (g) with Kc = 255 at 1000 K, if a reaction mixture initially contains a CO concentration of 0.1450 M and a Cl2 concentration of 0.176 M at 1000 K, what is the equilibrium concentration of CO?

For the reaction CO (g) + Cl2 (g) ⇌ COCl2 (g) with Kc = 255 at 1000 K, if the initial concentrations are [CO] = 0.1510 M and [Cl2] = 0.175 M, what is the equilibrium concentration of COCl2?

Given the equilibrium reactions:A(g) + B2(g) <==> AB(g) + B(g) with KC = 4AB(g) <==> A(g) + B(g) with KC = 0.5What is the equilibrium constant (KC) for the following reaction?2A(g) + B2(g) <==> 2AB(g)

What is the equilibrium expression for the reverse photosynthetic conversion of CO2 and O2, given the reaction: 6CO2(g) + 6H2O(l) ⇌ C6H12O6(s) + 6O2(g)?

Kc is 1.67 × 10^20 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O4^2-(aq) ⇌ [Fe(C2O4)3]^3-(aq). If 0.0100 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

Given that Kc is 1.67 × 10^20 at 25°C for the formation of the iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O4^2-(aq) ⇌ [Fe(C2O4)3]^3-(aq), and 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

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?