At 1 atm and 25 °C, NO2 with an initial concentration of 1.00 M is 0.0033% decomposed into NO and O₂. Calculate the value of the equilibrium constant for the reaction: 2NO₂ (g) 2NO(g) + O₂(g)

15.0 g of glucose reacts with oxygen in a 15.0 L container. At 250°C the system reaches equilibrium. At equilibrium it is determined that there are 5.25 mol of oxygen, 1.84 mol of carbon dioxide and 5.66 mol of steam. Calculate the value of the the equilibrium constant Kc. C6H12O6(s) + 602(g) = 6 CO2(g) + 6H2O(g) O9.64 x 10-5 O5.35 x 10 6 9- O1.87 x 105 O 0.0164 60.9

Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron/iron oxide catalyst. For the reaction: N₂(g) + 3H₂(g) → 2NH3(g) AH -92.22 kJ/mol At 300 °C the equilibrium constant for the reaction is 4.34 x 10-³. a) Is this reaction endothermic or exothermic? b) What effect would the following changes have on the equilibrium position. Write forward, reverse or no change: • Add some more nitrogen gas • Increase the volume of the reaction vessel • Decrease the temperature • Remove some hydrogen gas

Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g)      6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

What is the correct equilibrium constant expression for the balanced reaction shown below? 2 HCl (g) + I2 (s)   2 HI (g) + Cl2 (g)

Given the following equation: NH4 (aq) + NO2 (aq) → N2(g) + 2H2O (1) AH = -122.4 kJ/mol How would decreasing the pressure effect the equilibrium? It would cause the equilibrium to shift to the right, favoring the products or the forward reaction. It would cause the equilibrium to shift to the left, favoring the reactants or the reverse reaction. It would not effect the equilibrium.

The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K. Calculate Ke for this reaction at this temperature. C PC15 (g) → PC13(g) + Cl₂ (9) Kc = ||