Definition
Equilibrium Expression
ICE
Solving
Le Chatelier's Principle
100

A reaction where energy is located on the product side of a chemical equation.

Exothermic

100

What phases are included in the equilibrium expression?

gases and aqueous

100

What does "E" stand for in the ICE table?

equilibrium 

100

A reaction in a 1-L flask has initial concentrations of 0.20 mol PCl3(g) and 0.10 mol Cl2(g) produces PCl5. At equilibrium, the concentration of PCl3 was 0.12 mol. Find the value of Kc.

33

100

This stress is the only one which will actually change the K value?

temperature

200

This is the principle stating that a system in equilibrium will shift direction to balance any changes that are made.

Le Chatelier’s Principle

200

When is Keq reactant favored?

Keq < 1

200

A reversible reaction is indicated by ___ arrow.

double

200
An inorganic chemist studying the reactions of phosphorus halides, the equilibrium values were found to be 0.1050 mol of PCl5 , 0.0450 mol of Cl2 and 0.0450 mol of PCl3 in a 0.500-L flask at 250°. What is Kc value?

PCl5(g) <-> PCl3(g) + Cl2(g)  

3.8 x 10 -3

200

Describe where will the equilibrium shift to the chemical system A + B = C + D + 57kJ when the temperature is increased.

 shift left

300

A type of equilibrium when solids and liquids are part of the chemical reaction.

Heterogenous equilibrium
300

H2(g)+I2 (g) ⇄ 2HI (g)

[HI]2 / [H2][I2]

300

NH4CO2NH2(s) ⇄ 2NH3(g) + CO2(g)  

Write the Expression 

Keq = [NH3]2[CO2] 

300

For the reaction given below, 4.00 moles of A and 3.00 moles of B are initially placed in a 1.00 L container. At equilibrium, the concentration of A is 3.50 M. What is the value of K?

2A(g) + B(g) ⇌ C(g)

7. 4×10-3   

300

For the reaction X2(g) + 3Y2(g) = 2XY3(g) at equilibrium; what would be the result of increasing the pressure?

shift to the right

400

The thing you must do before predicting equilibrium shifts.

balance the equation

400

What is the equation for K for displacement reaction Zn (s) + 2 AgCl (aq) <--> 2 Ag (s) + ZnCl2(aq)

Kc= [ZnCl2] / [AgCl]2

400

A (g) + B (g) <---> C (g) Initially, 20 mol A and 15 mol B and 10mol C are put in a 5L flask. What are the initial concentrations of A, B, and C?

4M, 3M, 2M

400

If 0.050 M H2(g) and 0.050 M I2(g) are present initially and the equilibrium constant is 45, what is the HI concentration at equilibrium?

H2 (g) + I2 (g) ⇌ 2 HI (g)

0.077 M

400

5A (g) + 9D (g) <---> 6E (aq) + 3G (g) If we increase the volume, which way will the reaction shift?

left

500

What is the effect of catalyst in equilibrium?

Nothing. It will just speed up the reaction to reach equilibrium faster.

500

The Keq for this is [N2O4] / [NO2]2 . Write the reaction.

What is 2 NO2(g) ⇋ N2O4(g)

500

If 0.050 M H2(g) and 0.050 M I2(g) are present initially and the equilibrium constant is 45, what is the change in concentration of HI?

H2 (g) + I2 (g) ⇌ 2 HI (g)

+2x

500

The reaction SO3(g)+NO(g)<-->NO2(g)+SO2(g) has a Kc value of 6.78. The initial concentrations of NO and SO3 were both 0.03 M. Find the equilibrium concentrations of each component.

[SO3]=0.0083 M; [NO]=0.0083 M; [NO2]=0.022 M; [SO2]=0.022 M 

500

CO2 + H2O <---> H2CO3 If we dump in some H2CO3, where will the equilibrium shift to?

shift left

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