SIMULATION Equilibria and Volume I N204(g) 2 2 NO2(g) Equilibrium Concentration K = 0.880 NO2 0.339 M N204 0.131 M 0.5 1 1.5 2 2.5 3 3.5 Equilibrium Mole Fraction Volume 1.00 L NO2 0.722 Temperature 50 °C N204 0.278 0. 0.5 1.5 2 2.5 3 3.5 Calculate Clear Volume (L) Compare the system (still at 50 °C) with a volume of 1.0 L and with 3.0 L. What is the total amount of gas (mol) present in the container at each of these volumes? at 1.0 LI mol at 3.0 L mol Mole fraction Concentration (M) (103u/u)

A mixture of 0.5110 M CO and 0.3590 M Cl, is enclosed in a vessel and heated to 1000 K. CO(g) + Cl, (g)= COCI,(g) K. = 255.0 at 1000 K Calculate the equilibrium concentration of each gas at 1000 K. [CO] = M %3D [CI,] = M [COCI,] = M

Calculating equilibrium concentrations using the raction quotient

Calculate the composition of the gaseous mixture obtained when 2.15 mol of carbon dioxide is exposed to hot carbon at 810°C in a 2.45 L vessel. The equilibrium constant K. at 810°C is 9.00 for the reaction Co2(9) + C(s) - 20O(9) [CO2 M [CO] = M

Please provide detailed solution and give the explanation of the concept

Calculate the value of Kp for the equation C(s) + CO₂(g) 2 CO(g) given that at a certain temperature Kp Kp = ? C(s) + 2 H₂O(g)CO₂(g) + 2 H₂(g) H₂(g) + CO₂(g) H₂O(g) + CO(g) Kpl = 3.13 Kp2 = 0.625

As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C