Which of the following are good descriptions of what occurs at equilibrium? (Cho

Question

Which of the following are good descriptions of what occurs at equilibrium? (Choose all that apply)

a. The reaction quotient, Q, is equal to the equilibrium constant, K.   b. The forward and reverse rates of reaction are equal to one another.   c. The concentrations and pressures have stopped changing.   d. The reaction has stopped happening.   e. The amounts of products and reactants are equal.  


Under what conditions can you ALWAYS feel confident ignoring x in an ICE Table problem?

a. The initial conditions have no products.   b. The reaction is extremely product-favored.   c. The initial conditions have no reactants.   d. The initial conditions are very close to equilibrium   e. The reaction is extremely reactant-favored.  

The formation reaction of SF6 (g) proceeds accordingly:

S (s) + 3 F2 (g) <--> SF6 (g).

At equlibrium, a 5.0-L container holds 4.38 g elemental sulfur, 0.43 mol F2and 4.8 mol SF6. Calculate the equlibrium constant, KC for this reaction.





The next few questions deal with the following equilibrium in which nitric oxide decomposes into its component elements
2 NO (g) <--> O2 (g) + N2 (g)

The KP for this reaction is 2.4 x 1030 (that is not a typo... ten to the thirtieth!). Given a gas sample that is made up entirely of NO, what strategy would you use to determine the amount of NO present at equilibrium most quickly? (Hint: Assume your fancy graphing calculator with the "equation solver" feature was destroyed in a freak integrating accident)

a. Make an ICE Table and solve the resulting quadratic by hand.   b. Make an ICE Table, assume that the change will be negligible, and simplify the polynomial to simple cube root.   c. Make an IFICE Table, performing a stoichiometric shift ("FORCE") to get all products, then neglecting the change as the reaction reaches equilibrium from that state.   d. Sit on the ground and weep. (In all seriousness, don't click this one; it's wrong).  

Starting from a vessel containing an equimolar mixture of nitric oxide and nitrogen, each with a partial pressure of 1091 atm, determine the equilibrium PNO according to the reaction and KP given in Question 4.

Answer: Units:

Which direction would the reaction discussed above shift if each of the following changes were made to a vessel containing nitrogen, oxygen and nitric oxide at equilibrium (see Q#4)?

Preview columns:

• A fuel is burned inside the vessel, depleting the oxygen
• Helium is added to the vessel
• Vessel is compressed to half its original volume
• Fresh nitrogen is added to vessel

• no effect
• shift to left
• shift to right

Matching pairs: A fuel is burned inside the vessel, depleting the oxygen

Explanation / Answer

1. abc

2. c

3. 1509.3

4. c

5. 4.95*10^-25 atm

6. Shift to Right, Shift to Right, No effect, Shift to Left

7. Temperature increase leads to the reaction proceeding backwards. Thus, the reaction is Endothermic.

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