At 2000°C, K for the reaction N2(g) + O2(g) 2NO(g) is 0.01. Predict the direction in which the system will move to reach equilibrium at 2000°C if 0.4 moles of N2, 0.1 moles ofO2, and 0.08 moles of NO are placed in a 1.0-liter container.

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, Kc, for the following reaction is 55.6 at 698 K.H2 (g) + I2 (g) 2 HI (g)Calculate the equilibrium concentrations of reactants and product when 0.228 moles of H2 and 0.228 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = M [ I2 ] = M [ HI ] = M

The equilibrium constant (Kc ) for the reaction: PCl3 + Cl2 <=> PCl5 equals 51 at 235°C. If 0.648 mol  of phosphorus trichloride and 0.748 mol chlorine (Cl2) are added to a 9.00 L reaction vessel, what is the amount of moles of Cl2 at equilibrium  in the mixture at 235°C?

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

At 500K, the methanol decomposes according to the following reaction, CH3OH(g) = CO(g) + 2 H2(g) K= 9.60×10-2 Some methanol, CH3OH (molar mass: 32 g/mol), is placed into a rigid 2.00-L vessel, and the temperature is raised to 500K. If the concentration of H2 in the equilibrium mixture is 0.246M, what is the initial concentration of methanol? O A, 0.231 M Ов. 0.866 М OC 0.200 M OD. 1.109 M O E. 0.012 M

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…

A student ran the following reaction in the laboratory at 591 K:COCl2(g) CO(g) + Cl2(g)When she introduced COCl2(g) at a pressure of 0.380 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of Cl2(g) to be 0.247 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.

A chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.83. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, 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 C compound H₂ Cl₂ HCI H₂ CL₂ HCI H₂ CL₂ HCI pressure 4.00 atm 1.97 atm 3.36 atm 4.27 atm 2.82 m 3.84 atm 1.81 atm 3.69 atm expected change in pressure 1 increase O decrease decrease Of increase Of increase Ⓒ↓ decrease Of increase O decrease decrease O1 increase Ot increase O decrease Of increase O decrease Of increase O decrease decrease Of increase O (no change) (no change) O(no change) (no change) (no change) (no change) (no change) (no…

CS 2( g) + 3Cl 2( g) <=> CCl 4( g) + S 2Cl 2( g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.075 M, [Cl2] = 0.35 M, [CCl4] = 0.25 M, and [S2Cl2] = 0.45 M. What will be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, Cl2 = 0.15 M, CCl4 = 0.45M, and S2Cl2 = 0.31 M? I would like help with this problem I am solving for Kc and then Qc I believe. for Kc I set up the following equation using the molarity values in the brackets as (.25)(.45)/(.075)(.035)^3 and the Qc as (.45)(.31)/(.15)(.15)^3