Consider the following reaction: 2 NH3(g) 2 3 H2(g) + N2(g) Kc = 2.20 1.10 mol/L of nitrogen gas, 0.50 mol/L of hydrogen gas, and 0.25 mol/L of ammonia gas are added to an empty flask. Which way, if at all, will the reaction shift to reach equilibrium? The reaction will shift left to make more reactants and reach equilibrium. The reaction is already at equilibrium and, therefore, will not shift in either direction. The reaction will shift left to make more products and reach equilibrium. The reaction will shift right to make more products and reach equilibrium. O The reaction will shift right to make more reactants and reach equilibrium.

The chemical equation represents a reaction at equilibrium. 2SO3(g) = 2SO2 (g) +O2(g) Which of these shows the equilibrium constant expression for this chemical equation? A [O2][SO2]2/[SO3]2 B [O2]2[SO2]/2[SO3] C 2[SO3]/[O2]2[SO2] D [SO3]2/[O2][SO2]2

Consider the following equilibrium system: 2 NOCI(g) 2 2 NO(g) + Cl2(g) Kc = 57.0 Initially, only NOCI gas is placed in a flask. After equilibrium has been reached it is found that the concentration of the nitrogen monoxide gas in the flask is 1.14 mol/L. What is the initial molar concentration of the NOCI gas? Answer to three decimal places.

Consider the following reaction at equilibrium. What effect will removing some SO2 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The pressure of SO3 will increase The equilibrium constant will decrease. No change will occur since SO2 is not included in the equilibrium expression. The pressure of NO2 will increase. The reaction will shift to decrease the pressure.

1.QuestionGiven the reaction at equilibrium: 2 SO2(g) + O2(g) <--> 2 SO3(g) + heat Which change will shift the equilibrium to the right?     increasing the temperature increasing the pressure decreasing the amount of SO2(g) decreasing the amount of O2(g)

5.For the following equilibrium reaction:   Energy + 2AB2 (g)                   2 AB (g)  +  B2 (g)   where K = 55   What will happen to the amount of B2 (increase, decrease or stay the same) if   a catalyst is added   some AB is removed   temperature is increased   pressure is increased   the amounts of AB2 and AB are kept constant while the value of K is decreased

Consider the following equilibrium   If the equilibrium concentration of chlorine and phosphorous trichloride are 0.80 mol/L and 0.70 mol/L, respectively,find the equilibrium concentration of phosphorous pentachloride.

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease   (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease  (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e)…

Which is the correct equilibrium expression for the following reaction? Assume <--> is the equilibrium arrow, even though it doesn't really look like it!   2 F2 (g)  +  Xe (g)  <––>  XeF4 (g)

Consider the following equilibrium: 2 NH3(g) N2 (g) + 3 H2(g) Which of the following will happen when nitrogen gas (N₂) is added to the reaction mixture? --> The concentration of NH3 will decrease. The value of Keq will increase. The value of Keq will decrease. The concentration of H₂ will decrease.