The reaction N2(g) + 3 H2(g) ⇀↽ 2 NH3(g), has an equilibrium constant of 4.0 × 108 at 25◦C. What will eventually happen if 44.0 moles of NH3, 0.452 moles of N2, and 0.108 moles of H2 are put in a 10.0 liter container at 25◦C?  More N2 and H2 will be formed.  Nothing; the system is at equilibrium.  More NH3 will be formed.

CO2 and H, are allowed to react until an equilibrium is established as follows: CO2 (g) + H, (g)H,0 (g) + CO (g) What will be the effect on the equilibriumn of removing CO from the equilibrium mixture?

1. For the following reaction, initially you start with 1.33 mol of N2(g) and 2.80 mol of O₂(g) in a 2.50 L container. Determine all equilibrium concentrations if Keg is 8.68 at a temperature of 200K. 2NO(g) N₂(g) + O 206}

Gaseous NO is placed in a closed container at 477 oC, where it partially decomposes to NO2 and N2O: 3 NO(g)  1 NO2(g) + 1 N2O(g) At equilibrium it is found that p(NO) = 0.009840 atm, p(NO2) = 0.008270 atm, and p(N2O) = 0.008870 atm. What is the value of KP at this temperature?KP =

The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M

Please provide the correct answer. We typically use ICE tables with these problems but I need help

The following reaction is important in the production of sulfuric acid. 2SO2(g) + O2(g) 2SO3(g) At 627 °C, 0.0291 mol SO2, and 0.0148 mol O₂ are sealed in a 1.50 L reaction vessel. When equilibrium is reached at the temperature of 725 °C, the concentration of SO3 is determined to be 0.0175 M. What is the value of Ke for the reaction? Calculate the Kp for the reaction at 725 °C. (17 pts.)

Consider the following reaction where Kc PC15 (9) PC13 (g) + Cl₂ (9) A reaction mixture was found to contain 0.117 moles of PC15 (g), 0.0259 moles of PC13 (g), and 0.0368 moles of C1₂ (g), in a 1.00 liter container. Calculate c Qc² = = 0.0120 at 500 K. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? O The reaction must run in the forward direction to reach equilibrium. O The reaction must run in the reverse direction to reach equilibrium. O The reaction is at equilibrium.

Gaseous SO3 is placed in a closed container at 685 oC, where it partially decomposes to SO2 and O2: 2 SO3(g)  2 SO2(g) + 1 O2(g) At equilibrium it is found that p(SO3) = 0.001810 atm, p(SO2) = 0.007320 atm, and p(O2) = 0.009270 atm. What is the value of KP at this temperature? KP =  _______

What is the value of the equilibrium constant Kc of the reaction at the temperature of the vessel?