Question

QUESTION 1

1. What does “ICE” stand for, with respect to chemical reactions?

   		Immigration and Customs Enforcement
   		In Case of Emergency
   		Initial, Change, End
   		Initial, Change, Equilibrium
   		None of the above

1 points   

QUESTION 2

1. It is possible to solve for the value of K (the equilibrium constant) when:

   		the equilibrium concentrations of all reactants and products are known.
   		only the initial concentrations are known.
   		the initial concentrations of the reactants and the equilibrium concentrations of one or more products are known.
   		Choices a, b and c.
   		Choices a and c only.
   		Choices a and b only

1 points   

QUESTION 3

1. The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant (Hint: this was covered in class on Monday, Feb 25, or can be read about in section 15.3 of the online interactive textbook).
   
               H₂(g) + Br₂(g) ⇌ 2 HBr(g)        K_c = 3.8 × 10⁴
               2 HBr(g) ⇌ H₂(g) + Br₂(g)        K_c =   ?

   		1.9 × 104
   		5.3 × 10 -5
   		2.6 × 10 -5
   		6.4 × 10 -4
   		– 3.8 × 104

1 points   

QUESTION 4

1. Nitrogen and oxygen gas react to form nitric oxide, NO, at high temperature:
   
   N₂(g) + O₂(g) ⇌ 2 NO(g) K_p = 0.0025 at 2100°C
   
   
   Suppose that a sealed reaction vessel initially contains 1.3 atm N₂ and 1.3 atm of O₂. Using an ice table as part of your setup, calculate the partial pressure of NO at equilibrium at 2100°C.

   		0.0016 atm
   		0.0033 atm
   		1.3 atm
   		2.6 atm
   		None of the above

1 points   

QUESTION 5

1. Consider the following reaction:
   C + 2D --> CD₂
   A student places 0.50 M C and 1.0 M D into a flask and allows the reaction to come to equilibrium. If the equilibrium concentration of C is 0.45 M, what is the equilibrium concentration of D?

   		0.45 M
   		0.55 M
   		0.90 M
   		1.0 M
   		None of the above

Answer 1