The equilibrium constant, Kp. for the following reaction is 55.6 at 698 K: H2(g) +12(8) 2HI(g) Calculate the equilibrium partial pressures of all species when H₂ and I₂, each at an intitial partial pressure of 2.14 atm, are introduced into an evacuated vessel at 698 K. H₂ P 12 atm atm atm P HI

A mixture of 4.1 atm CO2, 2.1 atm H2, and 3.3 atm H₂O are added to a sealed 2.0 L vessel at 500 K and allowed to come to equilibrium according to the reaction below. CO₂(g) + H₂(g) = CO(g) + H₂O(g) Which direction must the reaction proceed based on the initial concentrations? 1. The reaction proceeds forward. 2. The reaction proceeds in reverse. 3. The direction cannot be determined.

The equilibrium reaction between dinitrogen tetraoxide, N2O4(g), and nitrogen dioxide, NO2(g), can be written as the following. N2O4(g)  2 NO2(g) Initially, 0.34 mol N2O4 were introduced into a 0.74 L vessel at 21°C. At equilibrium, 0.24 mol N2O4 were present. What is the value of Kc for this reaction at this temperature?

A mixture of 1.00 Atm of NO, 0.50 Atm of H2, and 1.00 Atm of N2 was allowed to reach equilibrium according to the reaction given below (initially there was no H2O). At equilibrium, the partial pressure of NO was found to be 0.62 Atm. Determine the value of the equilibrium constant, Kp, for the reaction: 2NO(g) + 2H2(g) ⇄ N2(g) + 2H2O(g)

At 1359 °C the equilibrium constant for the reaction: 2 BrCl(g) = Br₂(g) + Cl₂(g) is Kp = 2.11. If the initial pressure of BrCl is 0.00467 atm, what are the equilibrium partial pressures of BrCl, Br₂, and Cl₂? p(BrCl): = p(Br₂) = p(Cl₂): =

Consider the following reaction:   A2 (g) + B2 (g) ⇄ 2AB (g)  Kp = 25.6 The three species are mixed in a 5.000 L flask and have the following partial pressures:  PAB = 0.520 atm, PA₂ = 0.020 atm, PB₂ =  0.450 atm. What is the equilibrium partial pressure of AB in atm? Report your answer with four decimals. Enter numbers only; do not enter units.

At 1000 K, a sample of pure NO₂ gas decomposes: 2 2NO₂(g) = 2NO(g) + O₂(g) The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium. Part 1 of 2 What is the pressure of NO? Be sure your answer has the correct number of significant digits. Part 2 of 2 atm x10 atm X What is the pressure of NO₂? Be sure your answer has the correct number of significant digits. Ś x10

At a given temperature, the system N₂(g) + O₂(g) ≈ 2NO (g) is at equilibrium with Kp = 4.15.The system has the following partial pressures PN 2 1.23 atm and PNO = 5.35 atm. Determine the partial pressure of the oxygen gas present in this equilibrium mixture. -

Please don't provide handwritten solution ...

Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3)2 as (P NH3)2 . If either the numerator or denominator is 1, please enter 1   2 Co3O4(s)   ↔   6 CoO(s) + O2(g)