The following equation represents a reversible decomposition: CaCO3(s)⇌CaO(s)+CO2(g)CaCO3(s)⇌CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?

In the following gas phase reaction, Kc is much less than 1. At equilibrium, which of the following statements is true?COCl2(g) ⇌ CO(g) + Cl2(g)   A catalyst will increase the concentration of products formed. At equilibrium, the concentrations of reactants and products are equal. The concentration of products is much greater than the concentration of reactants. The concentration of reactant is much greater than the concentration of products. The concentrations of products and reactants are approximately equal.

Consider the equilibrium system described by the chemical reaction below. The decomposition of NOBr has a value Kc equal to 3.07 × 10⁻⁴ at 297 K. If an initial solution of 0.20 M NOBr decomposes, what will the concentration of NO be at equilibrium?   2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)

Consider the following reactions at equilibrium and determine which of the indicated changes will cause the reaction to proceed to the right. 1) 2 H2O(g)⇌ 2 H2(g) + O2(g) (remove water)2) H2(g) + I2(g) ⇌ 2 HI(g) (remove HI)3) CaCO3(s) ⇌ CaO(s) + CO2(g) (add CaCO3)4) N2(g) + O2(g) ⇌ 2 NO(g) (add O2)5) BaO(s) + SO3(g) ⇌ BaSO4(s) (add BaO) a.3, 4 b.2, 4 c.2, 3 d.1, 4 e.2, 3, 5

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

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. Deuterium, D, is an isotope of hydrogen.2 HD(g) ⇌ H2(g) + D2(g)              Kc = 0.286 H2(g) + 6 D2(g) ⇌ 12 HD(g) Kc = ?

The reduction of iron(III) oxide to iron during steel-making can be summarized by this sequence of reactions: 2C(s)+O2(g) ⇌ 2CO(g) K1 Fe2O3(s)+3CO(g) ⇌ 2Fe(l)+3CO2(g) K2 The net reaction is: 2Fe2O3(s)+6C(s)+3O2(g) ⇌ 4Fe(l)+6CO2(g) K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K1 and K2.

For the following reactions, determine whether the forward or reverse reaction is favored. 2 SO3(g) ⇌ 2 SO2(g) + O2(g) K = 2.5 × 1025   N2(g) + O2(g) ⇌ 2 NO(g) K = 4.1 × 10-31       H2(g) + Cl2(g) ⇌ 2 HCl(g) K = 5.1 × 108

The following reactions have the indicated equilibrium constants at a particular temperature:  N2 (g) + O2(g) ⇌ 2NO (g) Kc = 7.1 ×10−25 2NO (g) + O2 (g) ⇌ 2NO2(g) Kc = 6.4 × 109 Determine the value of the equilibrium constant for the following equation at the same temperature:  2NO(g) ⇌ N2(g) + O2(g)

Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(9) + 5O2(g) → 4NO(g) + 6H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound concentration at equilibrium NH, 1.8M 1.6M NO 1.7M AH,0 1.9M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. C. K x10