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 chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq)+CH3NH(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.80. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration HCH CO₂ 0.58 M ↑ increase ↓ decrease (no change) CH3NH2 0.57 M ↑ increase ↓ decrease (no change) A CH3CO2 1.09 M ○ ↑ increase ↓ decrease (no change) CH,NH, 1.28 M ○ ↑ increase ↓ decrease (no change) HCH,CO₂ CH3NH2 1.28 M ↑ increase ↓decrease (no change) 1.27 M ↑ increase ↓ decrease (no change) B CH,CO, 0.39 M ↑ increase ↓ decrease (no change) CHÍNH, HCH3CO2…

Consider the following chemical equilibrium: С (s)+ 2 Н, (g) — CH (g) Now write an equation below that shows how to calculate K, from K̟ for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K¸ = []

The equilibrium constant, K., for the following reaction is 1.29×102 at 600 K. COCI,(e)=CO(g) + Cl,(g) Calculate the equilibrium concentrations of reactant and products when 0.270 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COC,] = | M [CO] M [Cl,] M

Consider the following chemical equilibrium: 4 NH, (g) +3 0, (g)=2N, (g) +6 H,Oo (g) Now write an equation below that shows how to calculate K, from K, for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K_ = I

A mixture of 0.04289 mol of C2H4, 0.08501 mol of N2, 0.02401 mol of NH3, and 0.05848 mol of C6H6 is placed in a 1.0-L steel pressure vessel at 1258 K. The following equilibrium is established: 3 C2H4(g) + 1 N2(g)  2 NH3(g) + 1 C6H6(g) At equilibrium 0.005819 mol of NH3 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of C2H4, N2, NH3, and C6H6.Peq(C2H4) =  .Peq(N2) =  .Peq(NH3) =  .Peq(C6H6) =  .(b) Calculate KP for this reaction.KP =  .

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Use the References to access important values if needed for this question. The equilibrium constant, Kỵ, for the following reaction is 55.6 at 698 K. H₂ (g) + I2(g) → 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.384 moles of H₂ and 0.384 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H₂] = | M [12] [HI] = = M M

A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g) At equilibrium 0.01420 mol of H2 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4) = ______  .Peq(H2S) =  ______ .Peq(CS2) = ______  .Peq(H2) = _______  .(b) Calculate KP for this reaction.KP = _______  .

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: