2.21-L vessel was found to contain 4.18 x 10 -2 mol of CO 2, 2.81 x 10 -2 mol of CO, and 8.89 x 10 -3 mol of O 2 at 298 K. Is the system at equilibrium for the reaction 2CO 2 ⇌  2CO + O 2? If not, which direction must the reaction proceed to achieve equilibrium? ( Keq = 1.2 x 10 -13)

When the following process reaches equilibrium, does the system in question contain mostly reactants, mostly products, or fairly equal concentrations of both reactants and products? justify your answer. H2(g)+Br2(g)=2HBr(g)      Kc= 1.4x10-21 at 25°c

Do 6-10.

Consider the following reaction: CO (g) + 2 H₂ (9) CH3OH (g) A reaction mixture in a 5.21 - L flask at a certain temperature initially contains 27.4 g CO and 2.36 g H₂. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (K) for the reaction at this temperature. Kc = Submit ΠΑΠ ΑΣΦ 4 Request Answer ?

At 100° C, the Keq for the Haber process is 4,51 x 10-5: N2 + 3 H2        ó           2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium pNH3 = 105 atm, pN2 = 35 atm and pH2 = 495 atm     pNH3 = 35 atm, pN2 = 0 atm and pH2 = 595 atm   pNH3 = 26 atm, pN2 = 202 atm and pH2 = 42 atm   pNH3 = 105 atm, pN2 = 5 atm and pH2 = 55 atm

Consider the reaction 2 NH3 (g) ⇄ N2 (g) + 3 H2 (g). Suppose 6 moles of pure ammonia are placed in a 1.0 liter flask and allowed to reach equilibrium. If X represents the concentration (in M) of nitrogen present in the system once equilibrium is reached, which of the following will represent the concentration of ammonia in M? Group of answer choices 6–(X/2) 6–X 6–2X 6+2X 6+X

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease   (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease  (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e)…

Consider the following equilibrium: 2 NH3(g) N2 (g) + 3 H2(g) Which of the following will happen when nitrogen gas (N₂) is added to the reaction mixture? --> The concentration of NH3 will decrease. The value of Keq will increase. The value of Keq will decrease. The concentration of H₂ will decrease.

At a particular temperature, K = 7.3 x 10-6 for the following balanced reaction: 2N2O3 (9) + O2(g) → 2N2O4 (9) In an experiment in which 1.5 mol of N2O3 and 1.0 mol of O2 are mixed in a 1.5-L vessel, what are the equilibrium concentrations of all gases? [N203] = M [02] = M [N204] = M