The reaction between gaseous sulfur dioxide and oxygen is a key step in the industrial synthesis of sulfuric acid: 2SO2(g)+O2(g)⇌2SO3(g)2SO2(g)+O2(g)⇌2SO3(g) A mixture of SO2 and O2 was maintained at 800 K until the system reached equilibrium. The equilibrium mixture contained 5.0 × 10−2 M SO3, 3.5 × 10−3 M O2, and 3.0 × 10−3 M SO2. Calculate K and Kp at this temperature.

Nitrogen and hydrogen react according to the reaction below to form ammonia:N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) Kc = 4.51 x 10-5 at 450°C0.61M N2 and 0.74 M H2 are placed in a reaction flask. Calculate the equilibrium concentration of NH3.

Consider the following reaction between nitrogen and oxygen and its equilibrium constant at 2000 °C: N2(g) + O2(g) ⇌ 2 NO(g)Kc = 4.10 × 10−4 a)Is the formation of nitrogen monoxide favored at 2000 °C? Explain your answer without doing a calculation. b)What is the nitrogen monoxide concentration when a mixture of 0.40 mol of nitrogen gas and 0.30 mol of oxygen gas reaches equilibrium in a 2.0-L container at 2000°C?

Consider the reaction 2N2O(g) + 3O2(g) ⇌ 4NO2(g). Exactly 0.0567 mol of O2 and 0.013 mol of N2O were placed into a 500 mL flask. The equilibrium concentration of NO2 was 0.027 M. What is the value of K for this reaction?

For the reaction  2A(g) ⇌ 2B(g) + C(g),  Kc = 1.20 x10−7 at a given temperature.   If the initial concentration of A in a closed container is 0.610 M, what is the approximate equilibrium concentration of B?

An equilibrium mixture has 0.583 mol of sulfur dioxide and 0.240 mol of bromine in a rigid 1.25 -L container. The equilibrium concentration of SO2Br2(g) is 0.670 M. What is the value of the equilibrium constant, Kc for this reaction? Report your answer to THREE significant figures. SO2(g) + Br2(g) ⇌ SO2Br2(g)

What is the value of the equilibrium constant at 500 °C for the formation of NH3 according to the following equation? N2(g) + 3H2(g) ⇌ 2NH3(g) An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 °C was found to contain 1.35M H2, 1.15M N2, and 4.12×10−1M NH3.

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)

For the reaction 2CO2 (g) ⇌ 2CO (g) + O2 (g), Kc = 6.4 x 10-7. If 1.0 x 10-3 moles of CO2 is placed in a 1.0 liter vessel, what are the concentrations of all species at equilibrium?

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