(d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added? If more NO is added, [N2]    (Increases),(Decreases),(remains the same)  , [O2]    (Increases),(Decreases),(remains the same)  , and [NO] (Increases),(Decreases),(remains the same)     . (e) What will happen to the concentrations of N2, O2, and NO at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel? If the pressure is increased by reducing the volume of the reaction vessel, [N2]    (Increases),(Decreases),(remains the same), [O2]    (Increases),(Decreases),(remains the same), and [NO]  (Increases),(Decreases),(remains the same). (f) What will happen to the concentrations of N2, O2, and NO at equilibrium if the temperature of the system is increased? If the temperature is increased, [N2] (Increases),(Decreases),(remains the same), [O2] (Increases),(Decreases),(remains the same), and [NO] (Increases),(Decreases),(remains the same). (g) What will happen to the concentrations of N2, O2, and NO at equilibrium if a catalyst is added? If a catalyst is added, [N2] (Increases),(Decreases),(remains the same), [O2] (Increases),(Decreases),(remains the same), and [NO] (Increases),(Decreases),(remains the same).

Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed?  a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases

Hydrofluoric acid and water react to form fluoride anion and hydronium cation, like this: + HF(aq)+H,O(1)→F (aq)+H;O"(aq) At a certain temperature, a chemist finds that a 2.7 L reaction vessel containing an aqueous solution of hydrofluoric acid, water, fluoride anion, and hydronium cation at equilibrium has the following composition: compound amount HF 2.21 g H,0 857. g F 0.169 g H;O 0.141 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all?

(Data attached in picture)

Phosgene, COC2, is the chemical warfare gas commonly called mustard gas. It decomposes as 3) written below., At 900 C, the Ke - 0.83. Assume 0.400 mol of COCI2 are admitted into a 2.00 L container at 900C. What will be the equilibrium concentrations of CO, Cl2 and COCI2? USE THE QUADRATIC for this one. You will NOT need to use quadratic on a test but for take home problems it is OK, COC2 CO + Ck [CO]eq = (Ch]eq =. [COCb]eq =,

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all?

1. Please don't write on a paper. I can't understand handwritten.

At equilibrium, the concentrations in this system were found to be [N,] = [0,] = 0.100 M and [NO] = 0.400 M. N, (g) + 0,(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium is re-established? [NO]final = M