Chemical Equilibrium

I. A State of Dynamic Balance

Chemical Equilibrium

I. A State of Dynamic Balance-when a ________ results in the almost ________ conversion of ________ to ________, the ________ is said to go to __________, but _____ _________ ___ ____ go to __________, most _________ are __________

Chemical Equilibrium

I. A State of Dynamic Balance-as soon as the ________ ________ begins, the ____________ of the _________ go _____, and the _________ _____ goes _____ as the number of __________ per unit ____ goes _____

Chemical Equilibrium

I. A State of Dynamic Balance-as the _________ proceeds, the ____ of the ________ _________ continues to ________ and the ____ of the ________ ________ continues to ________ until the two _____ are _____, and the system has reached a state of ________ __________

Chemical Equilibrium

I. A State of Dynamic Balance-at ___________, the ____________ of the ________ and ________ are not _____, but _______, because the ____ of _________ of the ________ is _____ to the ____ of _________ of the ________

Chemical Equilibrium

II. Equilibrium Expressions and Constants

-while _____ chemical systems have little tendency to _____, and _____ chemical systems _____ readily and ___ to __________, _____ chemical systems reach a _____ of __________, leaving varying amounts of ________ ____________

-in 1864, Norwegian chemists ______ and _________ proposed the _______ ___________________, which states, at a given ___________, a chemical system may reach a _____ in which a particular _____ of _______ and _______ ____________ has a _______ value

Chemical Equilibrium

II. Equilibrium Expressions and Constants

-the _______ ________ for a _______ at __________ can be written ______________________________, where __ and __ are ________, __ and __ are ________, __, __, __, and __ are the ___________ in the ________ ________, and the __________ _______ __________ is

-___________ ________ with ___ values __ __ contain more ________ than ________ at ___________, while __________ ________ with ___ values __ __ contain more ________ than ________ at __________

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the homogeneous equilibrium for the synthesis of ammonia from nitrogen and hydrogen.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the equilibrium for the synthesis of Hydrogen iodide from iodine and hydrogen.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the equilibrium for the decomposition of Dinitrogen tetroxide into Nitrogen dioxide.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the equilibrium for the reaction of Carbon monoxide and Hydrogen which produces methane (Tetrahydrogen monocarbide) and water.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the equilibrium for the decomposition of Dihydrogen monosulfide into diatomic hydrogen and diatomic sulfur.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

-_________ in which all ________ and ________ are in the same ________ _____ are ____________, but ________ with _________ and ________ in _____ than ___ ________ _____ result in _____________ _________

Chemical Equilibrium

II. Equilibrium Expressions and Constants

-since ______ and _____ ________ and ________ don’t change ___________, (which is really their ______), if the ___________ remains ________, then in the ___________ _______ __________ for a ____________ ___________, the ___________ ________ only depends on the ______________ of the ________ and ________ in the _______ state of matter

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the heterogeneous equilibrium for the decomposition of Sodium Hydrogen carbonate into Sodium carbonate, Carbon dioxide, and water.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the heterogeneous equilibrium for the decomposition of Calcium carbonate into Calcium oxide and Carbon dioxide.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the complete, balanced thermochemical equation and equilibrium constant expression for the homogeneous equilibrium for the reaction of hydrazine (Tetrahydrogen dinitride) and Nitrogen dioxide, which produces nitrogen and water.

Name_________________

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the complete, balanced thermochemical equation and equilibrium constant expression for the homogeneous equilibrium for the reaction of Sulfur trioxide and Carbon dioxide, which produces Carbon disulfide and oxygen.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the complete, balanced thermochemical equation and equilibrium constant expression for the heterogeneous equilibrium for the reaction of monatomic Sulfur and fluorine gas, which produces Sulfur tetrafluoride gas and Sulfur hexafluoride gas.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the complete, balanced thermochemical equation and equilibrium constant expression for the heterogeneous equilibrium for the reaction of magnatite (Fe3O4) and hydrogen gas, which produces iron and water vapor.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the homogeneous equilibrium for the synthesis of ammonia and calculate the value of Keq when [NH3] = 0.933 M, [N2] = 0.533 M, and [H2] = 1.600 M.

Chemical Equilibrium

II. Equilibrium Expressions and Constants

Write the equilibrium constant expression for the homogeneous equilibrium for the decomposition of Sulfur trioxide into Sulfur dioxide and oxygen gas, and calculate the value of Keq when [SO3] = 0.0160 M, [SO2] = 0.00560 M, and [O2] = 0.00210 M.

Chemical Equilibrium

III. Le Châtelier’s Principle

A. Safety:

1. Hypothesis:

2. Prediction:

3. Gather Data:

B. Procedure:

3. Gather Data:

B. Procedure:

Chemical Equilibrium

III. Le Châtelier’s Principle

4. Analyze Data:

Chemical Equilibrium

III. Le Châtelier’s Principle

5. Draw Conclusions:

Chemical Equilibrium

III. Le Châtelier’s Principle

-in 1888, ________________________ discovered that there are ways to _______ _________ in order to make _________ more __________

-____________________ states that if a ______ (like a ______ in __________) is applied to a system at __________, the system _____ in the ________ that _______ the _____

-________ that reach __________ instead of going to __________ do not ________ as much

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

A. Changes in Concentration

Write the equilibrium constant expression for the equilibrium for the reaction of Carbon monoxide and Hydrogen to produce methane and water. Then, calculate the Keq value when [CO] = 0.30000 M, [H2] = 0.10000 M, and [CH4] = 0.05900 M, and [H2O] = 0.02000 M.

Chemical Equilibrium

III. Le Châtelier’s Principle

-_________ the ____________ of ___ _________ the _______ of _________ between ___ and ___, _________ the _____ of the _______ _______

A. Changes in Concentration

-the system responds to the ______ of the addition of _______ by forming more _______ to bring the system back into equilbrium

Chemical Equilibrium

III. Le Châtelier’s Principle

A. Changes in Concentration

Chemical Equilibrium

III. Le Châtelier’s Principle

A. Changes in Concentration -_________ the ____________ of a ________ causes __________ to _____ to the ____ to _______ the ____ of formation of ______

-_________ the ____________ of a ________ causes __________ to _____ to the ____ to _______ the ____ of formation of ______

Chemical Equilibrium

III. Le Châtelier’s Principle

A. Changes in Concentration

Predict what should happen to the following equilibrium if hydrogen bonding due to the addition of acetone binds water and effectively removes it from the products.

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

A. Changes in Volume -_________ the ______ of the _______ container, according to ______, ________ the ________, which in turn ________ the _____ of _________ between the ________ of the ________, _________ the _____ of the ________ _______

-the _____ in the _________ causes the _____ on the system to be _______ as for every __ _____ of _______ _______ _________, only __ _____ of _______ _______ are _________, which, according to ________, occupies __ the ______, which _________ the ________

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

Use Le Châtelier’s Principle to predict how each of these changes would affect the ammonia equilibrium system.

a. removing hydrogen from the system __________________________

b. adding ammonia to the system _______________________________

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

Use Le Châtelier’s Principle to predict how each of these changes would affect the ammonia equilibrium system.

1N2 (g) 3H2(g)+ 2NH3(g)

c. adding hydrogen to the system _______________________________

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

How would decreasing the volume of the reaction container affect each of these equilibria?

2SO2 (g) 1O2(g)+ 2SO3(g)a. _________________________

1H2 (g) 1Cl2(g)+ 2HCl(g)b. _____________________________

2NOBr(g) 1Br2(g)+2NO(g)c. _________________________

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

A. Changes in Temperature -while _______ in _____________ and ________ in _______ cause ______ in _________, they ___ ___ _______ the __________ _______, but a ______ in ___________ causes ______ in both the __________ ________ and the __________ _______

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

A. Changes in Temperature -since the _______ for making _______ has a _______ ____, the ________ _______ is _________, and the _______ _______ is __________, so ____ can be thought of as a _______ in the ________ _______ and a _______ in the _______ _______

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

A. Changes in Temperature -_________ the __________ is like _______ more _______ to the _______ in which _____ acts as a _______ and is _____ ___, in this case, the __________ _______ _______

-__________ shifts to the _____, _________ the ___________ of _______ because _______ is a _______ in the _______ _______

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

A. Changes in Temperature -_________ the __________ is like ________ _______ from the _______ in which _____ acts as a _______, in this case, the __________ _______ _______

-__________ shifts to the _____, _________ the ___________ of _______ because _______ is a _______ in the _______ _______

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

In the following equilibrium, would you raise or lower the temperature to get the following results?

a. increase the amount of CH3CHO______________________________

b. decrease the amount of C2H2 ________________________________

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

In the following equilibrium, would you raise or lower the temperature to get the following results?

1C2H2 (g) 1H2O(g)+ 1CH3CHO(g)

c. increase the amount of H2O _________________________________

ΔH0 = -151 kJ

Chemical Equilibrium

III. Le Châtelier’s Principle -stressors that cause a shift in equilibrium

In the following equilibrium, what effect does changing the volume of the reaction vessel have?

______________________________________________________________________________________________________________________________________________________________________________

In the following equilibrium, what effect does simultaneously increasing the temperature and the pressure have?

______________________________________________________________________________________________________________________________________________________________________________

Chemical Equilibrium

III. Le Châtelier’s Principle

A. Safety:

1. Hypothesis:

2. Prediction:

3. Gather Data:

3. Gather Data:

B. Procedure:

Chemical Equilibrium

III. Le Châtelier’s Principle

3. Gather Data:

B. Procedure:

Chemical Equilibrium

III. Le Châtelier’s Principle

4. Analyze Data:

A. The equation for the reversible reaction in this experiment is:

Chemical Equilibrium

III. Le Châtelier’s Principle

4. Analyze Data:

A. Use the equation to explain the colors of the solution in steps 1, 2, and 3

Chemical Equilibrium

III. Le Châtelier’s Principle

4. Analyze Data:

B. Explain how the equilibrium shifts when heat energy is added or removed.

5. Draw Conclusions:

Chemical Equilibrium

IV. Using Equilibrium Constants -when a ________ has a _____ ___, the __________ _______ contains _____ ________ than ________ at __________

-when a ________ has a _____ ___, the __________ _______ contains _____ ________ than ________ at __________

A. Calculating Equilibrium Concentrations -__________ ________ can also be used to ________ the __________ ____________ of any ________ in the _______

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations

At 1200 K, the Keq for the following reaction equals 3.933. What is the concentration of the methane produced, if [CO] = 0.850 M, [H2] = 1.333 M, and [H2O] = 0.286 M?

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations

At 1405 K, the Keq for the following reaction equals 2.27 x 10-3. What is the concentration of the Hydrogen gas produced, if [S2] = 0.0540 M, and [H2S] = 0.184 M?

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations

If Keq for the following reaction equals 10.5, what is the equilibrium concentration of Carbon monoxide, if [H2] = 0.933 M, and [CH3OH] = 1.32 M?

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

If the Keq for the following reaction equals 64.0, what are the equilibrium concentrations of I2, H2, and HI, if [I2]0 = 0.200 M, [H2]0 = 0.200 M and [HI] = 0.000 M?

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

1H2 (g) 2HI(g)1I2(g) +

[H2] [I2] [HI]

Initial

Change

Equilibrium

0.200 0.200 0.000

-1x -1x +2x

0.200 - 1x 0.200 - 1x 2x

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

If the Keq for the following reaction equals 16.0, what are the equilibrium concentrations of PCl3, Cl2, and PCl5, if [PCl5]0 = 1.00 M?

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

1Cl2 (g) 1PCl5(g)1PCl3(g) +

[PCl3] [Cl2] [PCl5]

Initial

Change

Equilibrium

0.00 0.00 1.00

+1x +1x -1x

0.00 + 1x 0.00 + 1x 1.00 – 1x

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

If the Keq for the following reaction equals 0.680, what are the equilibrium concentrations of COCl2, CO, and Cl2, if [CO]0 = 0.500 M and [Cl2]0 = 1.00 M?

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

1Cl2 (g)1CO(g)1COCl2 (g) +

[COCl2] [CO] [Cl2]

Initial

Change

Equilibrium

0.00 0.500 1.00

+1x -1x -1x

0.00 + 1x 0.500 - 1x 1.00 – 1x

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

If the Keq for the following reaction equals 36.0, what are the equilibrium concentrations of H2, Br2, and HBr, if [H2]0 = 0.250 M and [Br2]0 = 0.250 M?

[H2] [Br2] [HBr]

Initial

Change

Equilibrium

Name_________________

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

[H2] [Br2] [HBr]

Initial

Change

Equilibrium

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

If the Keq for the following reaction equals 20.0, what are the equilibrium concentrations of H2, Cl2, and HCl, if [H2]0 = 1.00 M and [Cl2]0 = 2.00 M?

[H2] [Cl2] [HCl]

Initial

Change

Equilibrium

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

[H2] [Cl2] [HCl]

Initial

Change

Equilibrium

Chemical Equilibrium

IV. Using Equilibrium Constants

A. Calculating Equilibrium Concentrations from Initial Concentrations Using ICE (Initial, Change, Equilibrium)

Chemical Equilibrium

V. Solubility Equilibria -like a few _________ _________ that go to _________, upon __________, some ______ __________ _________ completely into _____

-some _____ __________, however, are only ________ _______, and quickly reach a ________ __________

Chemical Equilibrium

V. Solubility Equilibria -in the __________ _______ __________, ______ ______ is a _____, so the _______ is _______, and can be combined with the ___ value to form the ________ _______ _______

Write the solubility constant expression for the following solubility equilibrium:

Chemical Equilibrium

V. Solubility Equilibria

A. Calculating Solubilities from Solubility Product Constants

What is the solubility, in M, of Silver iodide at 298 K?

Chemical Equilibrium

V. Solubility Equilibria

A. Calculating Solubilities from Solubility Product Constants

What is the solubility, in M, of Copper(II) carbonate at 298 K?

Chemical Equilibrium

V. Solubility Equilibria

B. Calculating Ion Concentration from Ksp

What is [OH-] at 298 K in a saturated solution of Mg(OH)2 at equilibrium?

Chemical Equilibrium

V. Solubility Equilibria

B. Calculating Ion Concentration from Ksp

What is [Ag+] at 298 K in a saturated solution of AgBr at equilibrium?

Chemical Equilibrium

V. Solubility Equilibria

B. Calculating Ion Concentration from Ksp

What is [F-] at 298 K in a saturated solution of CaF2 at equilibrium?

Chemical Equilibrium

V. Solubility Equilibria

C. Predicting Precipitates -besides being used to calculate the _________ of an _____ _________ and the ___________ of ____ in a _________ _______, ___ values can be used to _______ if a _________ will form if ___ _____ __________ are mixed

Predict whether PbCl2 will form as a precipitate if 100 mL of 0.0100 M NaCl is added to 100 mL of 0.0200 M Pb(NO3)2:

-the ____________ of the ______ ________ allow you to _______ the ____________ of ____ and ___ ions in the _____ _________, which when _________ together, determine the ___ _______, or ___

Chemical Equilibrium

V. Solubility Equilibria

C. Predicting Precipitates

Predict whether PbCl2 will form as a precipitate if 100 mL of 0.0100 M NaCl is added to 100 mL of 0.0200 M Pb(NO3)2:

Chemical Equilibrium

V. Solubility Equilibria

C. Predicting Precipitates -if the ___ is ___ the ___, the _______ is __________, and a _________ ____ ___ ____, and if the ___ is ___ the ___, the _______ is _________ and ___ ______ will occur, but if ___ is ___ the ___, a __________ will form, reducing the ___ ___________ until ___ ___ ___, and the system arrives at __________ and the _______ becomes ________

Chemical Equilibrium

V. Solubility Equilibria

C. Predicting Precipitates

Predict whether Ag2SO4 will form as a precipitate if 500 mL of 0.010 M AgNO3 is added to 500 mL of 0.25 M K2SO4:

Chemical Equilibrium

V. Solubility Equilibria

C. Predicting Precipitates

Predict whether a precipitate will form if 200 mL of 0.20 M MgCl2 is added to 200 mL of 0.0025 M NaOH:

Chemical Equilibrium

V. Solubility Equilibria

D. Common Ion Effect -the ________ of _______ in _____ is ________ mol/L, which means that you can ________ ________ of _______ in ____ L of _____ _____, but _________ of _______ will ____ _______ in ____ L of a ______ solution of _______, because of the ________ ___ ______

-since the _______ of the ____________ of both ____ is _____ to a _______, (the _________ _______ _______), if _______ goes __, _____ must go _____

Chemical Equilibrium

V. Solubility Equilibria

D. Common Ion Effect -adding a _______ to an __________ that contains a ________ ___ _______ the ________ of a _________ containing that ___, or, according to _____________ ________, stresses the __________ and causes the _______ to _____ the __________ in the _______ that _______ the ______

Chemical Equilibrium

A. Safety:

1. Hypothesis:

2. Prediction:

3. Gather Data:

Chemical Equilibrium

V. Solubility Equilibria

B. Procedure:

1. Using a pipette, place 10 drops of AgNO3 solution into test well A1 of a 20-well microplate. Place 10 more drops of the same solution in test well A2.

3. Gather Data:

B. Procedure:

3. To test well A2 only, add 10 drops of Na2S solution. Record observations______________________________

2. Add 10 drops of NaCl solution to both test well A1 and test well A2. Record observations___________________

Chemical Equilibrium

V. Solubility Equilibria

4. Compare the contents of test wells A1 and A2. Record observations_____________________________________

4. Analyze Data:

A. Write the complete thermochemical equation for the reaction that occurred in Step 2.

Chemical Equilibrium

V. Solubility Equilibria

B. Write the net ionic equation for the reaction in Step 2.

C. Write the equation for the solubility equilibrium that was established in test wells A1 and A2 during Step 2.

D. Write the solubility constant expression for the equilibrium established in test wells A1 and A2 during Step 2.

E. Write the equation for the solubility equilibrium that was established in test well A2 during Step 4.

4. Analyze Data:

F. Match the chemical formula of each precipitate with its color.

Chemical Equilibrium

V. Solubility Equilibria

G. Compare the two Ksp values for the two precipitates. Infer which is the more soluble.

H. Use Le Châtelier’s Principle to explain how the addition of Na2S in Step 4 affected the equilibrium in test well A2.

4. Analyze Data:

Chemical Equilibrium

V. Solubility Equilibria

I. Calculate the molar solubilities of both precipitates in the experiment. Which of the precipitates is more soluble?