The reaction 2 H₂O(g) 2 H₂(g) + O₂(g) proceeds at an unspecified temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.015 bar, 0.0080 bar, and 0.0085 bar, respectively. What is the value of the equilibrium constant in terms of partial pressures at this temperature? Kp =

A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established:   1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g)Peq   the equilibrium partial pressures of CH4, H2S, CS2, and H2. (CH4) =  7.5Peq(H2S) = 5.35Peq(CS2) = 6.42Peq(H2) =   1.5195   At equilibrium 0.01420 mol of H2 is found in the reaction mixture. Calculate KP for this reaction.KP = _____  .

For the reaction X(9) + 4Y(g) = 3Z(g) K, = 2.51 × 10-2 bar-2 at a temperature of 361 °C. Calculate the value of Kc. Express your answer numerically.

Consider the following reaction:CH3OH(g) CH2O(g) + H2(g) K = 3.29 x 10−11a. If 14.4 g of CH3OH(g) is added to a 1.50 L container at 298 K, calculate the equilibriumconcentrations of all gases b. Without doing any calculations, predict what happens if the reaction is put in a 2.00 Lcontainer instead of a 1.50 L container. c. . Without doing any calculations, predict what happens if H2SO4 (a catalyst) is added

calculate the value of the reaction quotient. determine is the system is at equilibrium. if not which direction must the reaction proceed to reach equilibrium

The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation K₂ = K. (RT)An where R = 0.08206 L-atm/(K-mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N₂(g) + 3H₂(g) = 2NH3(g) for which An=2-(1+3) = -2.

Consider the reaction: 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br₂) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBr at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L･bar/mol･K and MW of Br₂ is 159.808 g/mol.) Calculate the Kp.

The formation of ammonia gas from molecular nitrogen and molecular hydrogen gas has the following Kp value. Get the value for the reverse reaction.

At high temperature, HCl and O2 react to give Cl2 gas: 4HClg) + O2(g) ⇌  2 Cl2 (g) + 2H2O(g) If HCl at 2.30 bar and O2 at 1.00 bar react at 750K, the equilibrium pressure of Cl2 is measured to be 0.93 bar. Determine the value of Keq at 750 K. Use a systematic approach to include setting up an ICE table, constructing equilibrium constant expression and show calculation involved.

Calculate the reaction quotient, QR for the following reactions and conditions:    2 NOCl(g)      :   KP = 2.5 x 103;  PNO = 0.0032 atm; PCl2 = 0.023 atm; PNOCl = 0.210 atm   2 NH3(g) N2(g) + 3H2(g)     :   KP = 17.0;  PNH3 = 0.13 atm; PN2 = 0.34 atm; PH2 = 1.1 atm