4 of 4 Equilibrium Practice Problem #2 When hydrogen and iodine are placed in a closed container at 440°C, they react to form hydrogen iodide. Hz + làm 2 HI At this temperature, the equilibrium constant, Keq is 49.7. Determine the concentrations of all entities at equilibrium if 4.00 mol of hydrogen and 2.00 mol of iodine are placed in a 2.00 L reaction vessel. (1.07 molt; 0.07 molt; 1.87 molt) ( 192

1.1 2NH3(g) AH is negative (b) N2(g) + 3H2 (g) From the given reaction at equilibrium above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of ammonia (b) Increasing the pressure I (c) Increasing the temperature (d) Adding a catalyst (e) Increasing the concentration of hydrogen will shift the equilibrium position to the left

What’s the equilibrium constant (K), for the following equation, if you have at equilibrium 0.25 mol/L of NH3 , 1.516 mol/L of H2 and 0.505 mol/L of N2 when it comes to equilibrium? 2 NH3(g)à 3 H2(g)+ N2(g) Table NH3 H2 N2 Initial 1.261 M 0 M 0 M Change -2x +3x +x Equilibrium 0.25 M 1.516M 0.505M

answer c