We have used the equilibrium expression, relating equilibrium constant and concentrations to calculate equilibrium constants. We can also calculate equilibrium concentrations using the equilibrium expression. Carefully sort out the known quantities and the unknown to solve the following.Determine the equilibrium concentration of the reactant, N2O4(g), for the following reaction system at 25°C :  N2O4 (g)   ⇋    2NO2 (g)    At 25°C, Kc = 0.040At equilibrium at 25°C,  [NO2] = 0.107 mol/L.(write the equilibrium expression first, rearrange carefully)The equilibrium concentration of N2O4(g) in mol/L is Question 2Select one:a.2.68b.0.286c.3.49d.0.374e.0.0286

At a particular temperature, K = 4.0 x 10-7 for thereaction:N2O4(g) <-->2NO2(g)In an experiment, 1.0 mol N2O4 is placedin a 10 L vessel. Calculate the concentrations ofN2O4 and NO2 when this reactionreaches equilibrium.

A solution is made by mixing 30.0 mL of 0.150M (mol/L) compound A with 25.0 mL of 0.200M (mol/L) compound B. At equilibrium, the concentration of C is 0.0454M. Calculate the equilibrium constant, K, for this reaction.A (aq) + 2B (aq) <---> C (aq)The initial concentrations of A and B are not 0.150 M and 0.200 M

Calculate ΔG° for the reaction below under standard conditions at 25°C.  2S(s) + 3O2(g) + 2H2O(l) → 2H2SO4(l) ΔH° = -1056 kJ/molΔS° = -505 J/molHint: Pay attention to units of ΔH° and ΔS°

The equilibrium constant for the reaction below is 7.2 × 10-4at 298 K and 1 atm.HNO2(aq) + H2O(l) NO2-(aq) + H3O+(aq)When [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0× 10-5 M, calculate ΔG.

The equilibrium constant, KC, for the following reaction is 2.5 × 10-3N2(g) + O2(g) ⇌ 2NO(g)If [N2]eq = 0.75 M and [NO]eq = 0.090, then [O2]eq