A gaseous mixture containing 0.15 M CO, 0.15 M H2, and 0.0035 M CH3OH, is placed in a 50.0-L vessel at 500 K. What will be the direction of the reaction if this mixture goes to equilibrium? The equilibrium constant equals 0.61 at 500 K. Show calculation for full credit. CO(g) + 2H2(g) → CH3OH(g)

Consider the reaction of N₂O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O₂ and 0.200 mol N₂O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 0.0100 0.0410 0 -0.0100 0.0710 1 2 N₂O(g) + 3 O₂(g) = 4 NO2(g) 2N₂O(g) 0.0560 -0.0050 0.0360 0.200 0.0050 0.180 + -1.00 0.0150 30₂(g) 2 -0.0560 -0.0150 0.0200 0.210 4NO₂(g) RESET -0.0200 0.190 +

Bromine monochloride is synthesized using the reaction Br, (g) + Cl, (g) = 2BrCl(g) Кр 1.1 x 10-4 at 150 K A 206.0 L flask initially contains 0.965 kg of Br, and 1.012 kg of Cl,. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: g What is the percent yield of BrCl? percent yield:

Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)

Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.110 M and [12] = 0.270 M. The equilibrium constant Kc for the reaction H2(g) +I2(g) = 2 HI(g) is 57.0 at 700 K. Part A Calculate the equilibrium concentrations of H2. Express your answer to three decimal places and include the appropriate units.

At a certain temperature , the given reaction has an equilibrium constant of K_{p} = 363; PCl 3 (g)+Cl 2 (g) rightleftharpoons PCl 5 (g); PC*l_{5} is placed in a sealed container at an initial pressure of 0.0640 bar. What is the total pressure at equilibrium ? Use the quadratic formula in solving steps.

A closed 1.00 L system initially containing 0.00200 mol H₂ and 0.00500 mol 1₂ at a given temperature is allowed to reach equilibrium Analysis of the equilibrium mixture shows that the amount of HI present at equilibrium is 0.00371 mol. Calculate the Kc at this temperature for the reaction. State whether the equilibrium is product-favored or reactant- favored at this temperature. H₂(g) +1₂(g) 2H1(g) Kc 31: The equilibrium is product-favored. Kc 31: The equilibrium is reactant-favored. Kc 0.032; The equilibrium is reactant-favored. Kc - 0.032; The equilibrium is product-favored.

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.700 M, B] = 0.950 M , and [C = 0.500 M. The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.510 Mand C = 0.690 M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically.

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.400 M , [B] = 1.40 M , and [C] = 0.300 M. The following reaction occurs and equilibrium is established: %3D %3D A + 2B = C At equilibrium, [A] = 0.270 M and [C = 0.430 M. Calculate the value of the equilibrium constant, K. Express your answer numerically. • View Available Hint(s) ΑΣφ Kc =

A mixture of ammonia, nitrogen, and hydrogen was allowed to come to equilibrium at 900K. 2NH3 ⇌ 2H2 + N2        Kc = 0.0076. An analysis of the mixture at equilibrium revealed 0.31 M of H2 and 1.8 M of NH3. Determine the equilibrium concentration of N2 (in M) in this mixture. (use 2 significant figures)