KpKp

Consider the reaction: N₂ (9) +202 (g) ⇒ N₂O4 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: N₂O4 (9) 2NO₂(g) K₁ 1/2N₂(g) + O₂(g) NO₂ (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K =

Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(9) + 2 H,O(g) 2 NO(g) + 2 H2(g) → Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound pressure at equilibrium N2 92.2 atm H,O 76.1 atm NO 19.3 atm H2 33.6 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0

Write the Kc and Kp (if applicable) expressions for the following heterogeneous equilibrium reactions:   a)2Hg(l)+O2(g)⇌2HgO(s)   b)C(s)+2H2(g)⇌CH4(g)   c)2Mg(s)+O2(g)⇌2MgO(s)

What is the value of the equilibrium constant for the reaction below if the partial pressures at equilibrium are [PH3] = 0.022 atm, [P2] = 0.289 atm, and [H2] = 0.867 atm at 873 K? 2 PH3 (g) ⇌ P2 (g) + 3 H2 (g)

As shown in Table 15.2 in the textbook, KpKp for the equilibriumN2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g)is 4.51×10−54.51×10−5 at 450 ∘C∘C. For each of the mixtures listed here, indicate whether the mixture is at equilibrium at 450 ∘C∘C. If it is not at equilibrium, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. A. 98 atmatm NH3NH3, 45 atmatm N2N2, 55 atmatm H2H2 98  , 45  , 55   a. yes, mixture is at equilibrium b. no, mixture must shift toward products to achieve equilibrium c. no, mixture must shift toward reactants to achieve equilibrium B.57 atmatm NH3NH3, 143 atmatm N2N2, no H2H2 57  , 143  , no  a.yes, mixture is at equilibrium b.no, mixture must shift toward products to achieve equilibrium c.no, mixture must shift toward reactants to achieve equilibrium

Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(g)+H2O(g)⇌3H2(g)+CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760. °C? Enter your answer with 3 sig figs.