2 SO3(g)           ⇄        2 SO2(g)           +          O2(g) 4.00 moles of SO2 and 5.00 moles O2 are present in a 2.00 L container at 100oC and are at equilibrium. Calculate the equilibrium concentration of SO3 and the number of moles SO3 present if the Keq = 1.47 x 10-3.

35 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 3.01 × 10³ at 900 K. If an initial mixture of 0.0216 mol SO2 and 0.0148 mol O2 reacts in a 1.0 L vessel, what will be the concentration of SO3 at equilibrium? 2 SO:(g) + O2(g)= 2 SO:(g) 1 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. 2 SO:(g) O:(g) + 2 SO:(g) Initial (M) 0.0216 0.0148 Change (M) 0.0216 - 2x 0.0148 - x Equilibrium (M) 5 RESET 0.0216 0.0148 1.0 +x +2x -2x 0.0216 + x 0.0216 + 2x 0.0216 - x 0.0216 - 2x 0.0148 + x 0.0148 + 2x 0.0148 - x 0.0148 - 2x

A mixture of ammonia, nitrogen and hydrogen was allowed to come to equilibrium at 900 K. 2NH3 = 3H2 + N2 Ke = 0.0076 An analysis of the mixture at equilibrium revealed 0.31 M of H2 and 1.8 M of NH3. Determine the equilibrium concentration of N2 (in M) in this mixture. (with 2 significant figures)

Consider the following system at equilibrium where AH 2NOBr(g) 2NO(g) + Br₂ (9) O increases O decreases O remains the same The value of Qc O is greater than Ke is equal to Ke O is less than Ke If the VOLUME on the equilibrium system is suddenly increased at constant temperature: The value of Ke The reaction must O run in the forward direction to reestablish equilibrium. O run in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. = The number of moles of Br₂ will O increase O decrease O remain the same 16.1 kJ, and K = 6.50 × 10-³, at 298 K: -3