The equilibrium constant, Kp, for the reaction PCl5 (g) > PCl3 + Cl2 is 1.26 at 250°C. The reaction is started with PCl5, PCl3, and Cl2 at 0.01, 0.2 and 0.5 atm at 250°C. When will the reaction come to equilibrium?

A chemical engineer is studying the following reaction: HCH;CO,(aq)+CH;NH,(aq) → CH;CO,(aq)+CH,NH,(aq) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.73. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound concentration expected change in concentration vessel HCH;CO, 1.18 M f increase I decrease (no change) CH, NH, 0.97 M f increase OI decrease O (no change) A CH,CO, 0.39 M f increase O I decrease (no change) + CH,NH, 0.39 M f increase Ot decrease (no change) HCH,CO, 1.15 M f increase OI decrease O (no change) CH,NH, 0.88 M t increase I decrease (no change) В CH,CO, 0.86 M f increase OI decrease (no change) CH,NH,…

Consider the following equilibrium process at 686 degrees celsius. CO2 (g) + H2 (g) ---> CO (g) + H2O (g) The equilibrium concentrations of the reaction species are [CO]= 0.0510 M, [H2]= 0.0410 M, [CO2]= 0.0840 M, and [H2O]= 0.0390 M. a) alculate Kc for the reaction at 686 degrees celcius. Round your answer to 3 significant figures. b) If we add CO2 to increase its concentration to 0.420 M, what will the concentration of all the gases be when equilibrium is reestablished? [CO2]=  M.  Round your answer to 3 significant figures. c) [H2] =  M. Round your answer to 2 significant figures. d) [CO]=  M. Round your answer to 2 significant figures. e) [H2O]=  M.  Round your answer to 2 significatnt figures

At 2516 °C the equilibrium constant for the reaction: 2 BrCl(g) Br₂(g) + Cl₂(g) is Kp = 0.863. If the initial pressure of BrCl is 0.00277 atm, what are the equilibrium partial pressures of BrCl, Br₂, and Cl₂? p(BrCl) = p(Br₂) = p(Cl₂) =

Can you provide an explanation? And show the steps

A reaction vessel is charged with 0.50 atm of A and 0.300 atm of B. Once the reaction reaches equilibrium, what is the equilibrium partial pressure of B? Kp for this reaction is 67.2 A(g) - 2 B (g)

A chem ngineer is studying the following reaction: 4 HCl(g)+O,(g) – 2 H,0(g)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0040. The engineer charges ("fillsf) four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the co mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel HCl 8.71 atm Ot increase O! decrease O (no change) 02 8.13 atm O t increase OI decrease O (no change) H,0 3.63 atm Ot increase OI decrease (no change) I decrease (no change) Cl, 1.91 atm ease I decrease (no change) 7,61 atm t increase HCI I decrease O (no change) 7,86 atm O f increase 0, I decrease O (no change) 4.18 atm t increase H,0 I decrease (no change) t increase 2.46 atm Cl, I decrease O (no…

3 A + 2 B → 1 CCalculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 6.87 M and [B] is 6.38 M. After the reaction has reached equilibrium, [C] is 1.47 M. Unfortunately, significant figures cannot be taken into account here, so please ignorethem this time.