At a particular temperature, K 2.0 x 10 0 for the reaction 2 CO2 (9) =2 CO(g)+ O2(9) If 2.5 moles of CO2 is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species. [CO2] =0.5 M (CO) = %3D

A chemical engineer is studying the following reaction: N2(9)+3H,(g) → 2NH,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.00029. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, 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 compound pressure expected change in pressure vessel N2 52.94 atm f increase OI decrease (no change) H2 23.44 atm O t increase OI decrease O (no change) A NH3 14.08 atm O t increase I decrease (no change) N2 47.16 atm O f increase I decrease (no change) В H2 20.07 atm O f increase O I decrease (no change) NH3 11.95 atm O f increase OI decrease (no change) N2 47.80 atm O f increase OI decrease (no change) H2 21.97 atm O f increase OI decrease (no…

The equilibrium constant, K., for the following reaction is 77.5 at 600 K. Co(g) + C,(g)=COC»(g) Calculate the equilibrium concentrations of reactant and products when 0.593 moles of CO and 0.593 moles of Cl, are introduced into a 1.00 L vessel at 600 K. [CO] M [Cl,] M [COCI,] =

A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.00014. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, 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 vessel A B C compound N₂ H₂ NH3 N₂ H₂ NH₂ N₂ H₂ NH₂ pressure 32.70 atm 49.38 atm 23.45 atm 33.09 atm 50.55 atm 22.67 atm 33.10 atm 50.59 atm 22.64 atm expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase O ↑ increase ↑ increase ↑ increase ↑ increase decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease decrease ↓ decrease decrease decrease (no change) (no change) (no change) (no change) (no change) O (no change) (no…

The equilibrium constant for the reaction                         NO(g) + NO2(g)  ⇆  N2O3(g) is Kp = 5.8 at 107oC. If 5.1 Atm of N2O3 is placed in an evacuated container at 107oC what is the partial pressure of NO (in Atm) at equilibrium?

The equilibrium constant for the reaction N2 + 3H2 <=> 2NH3 is Kp = 4.34 * 10-3 at 300 °C. Pure NH3 is placed in a 1.00-L flask and allowed to reach equilibrium at this temperature. There are 1.05 g NH3 in the equilibrium mixture. What was the initial mass of ammonia placed in the vessel?

Bromine monochloride is synthesized using the reaction Br₂ (g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 208.0 L flask initially contains 0.953 kg of Br₂ and 1.184 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? percent yield: 6.D g %

Daniela A chemical engineer is studying the following reaction: 2 H,S(g)+302(g) → 2 SO2(g)+2H,O(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, 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 expected change in pressure pressure H, S 1.52 atm O t increase O I decrease O (no change) 0, 8.80 atm O t increase O I decrease O (no change) A so, 9.53 atm O t increase O I decrease O (no change) H,0 5.94 atm O f increase O I decrease O (no change) H, S 0.79 atm O t increase O I decrease O (no change) 6.91 atm Ot increase O l'decrease O (no change) so, 8.61 atm O t increase O I decrease O (no change) H,0…

The equilibrium constant Ke for the reaction PCI3 (9) + Cl2 (g) = PCI, (g) equals 3.5 at 310°C. a A sample of 38.1 g of PCl; is placed in a 2.1 L reaction vessel and heated to 310°C. What are the equilibrium concentrations of all of the species? [PCI5] = | M [PCI3] = | |M [CL] = [ M

The equilibrium constant, K., for the following reaction is 83.3 at 500 K. PC13(g) + C2(g)=PC!{(g) Calculate the equilibrium concentrations of reactant and products when 0.380 moles of PC13 and 0.380 moles of Cl, are introduced into a 1.00 L vessel at 500 K. [PC13] =| M [Cl2] M [PClg] = | M