For this reaction: 2O2(g) <-----> 2CO(g) + O2(g) K equals 2.35 x 10-5 at a particular temperature. If 3.5 moles of CO2 are initially placed into a 3.0L flask, calculate the equilibrium concentrations of all species.

Use the References to access important values if needed for this question. The equilibrium constant, Kc, for the following reaction is 0.0290 at 1150 K. 2SO3 (g) ⇒ 2SO2 (g) + O2 (9) If an equilibrium mixture of the three gases in a 18.0 L container at 1150 K contains 0.356 mol of SO3(g) and 0.469 mol of SO2, the equilibrium concentration of O₂ is M. An error has been detected in your answer. Check for typos,

A student ran the following reaction in the laboratory at 672 K: 2NH3(g)     N2(g) + 3H2(g) When she introduced 6.42×10-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 9.09×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HF (aq) + OH- (aq)F- (aq) + H2O (l)   K =

A student ran the following reaction in the laboratory at 431 K: PCI 5(9) PC13(g) + Cl₂(9) When she introduced 2.02 moles of PCI5(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.08x10-² M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.