Chapter 9
Chapter 10
Chapter 11
Chapter 12
100

Solve the ideal gas law equation for pressure.


P = nRT/volume


100
Sublimation refers to what phase change?

solid to gas

100

Bonus!

100
100

As the activation energy for a reaction increases, the speed of a reaction

Decreases


200
Dalton's Law states

Total pressure = [partial pressure of gas A] + [partial pressure of gas B] + ...

200
The boiling point occurs when

the vapor pressure = external pressure of the atmosphere

200

Ionic solutes are more soluble in nonpolar or polar solvents?

Polar

200

Which of the following decreases the reaction rate?

More than one correct answer

I. Decrease concentration of the reactants

II. Increase temperature

III. Adding a catalyst 

IV. Increasing the surface area (if reactant is a solid)

II

300

Bonus!

100

300

Which of these statements is false?

I. Solids have a fixed shape.

II. Gases fill their container.

III. There is little free space between solid particles.

IV. Gas particles have the lowest kinetic energy of any of the phases.

V.  Liquids have a fixed volume and have more kinetic energy than solids. 

IV

Kinetic energy = molecular movement of the particles

Higher KE = higher temperature

Gas > liquid > solid in terms of kinetic energy.

300
Substance A has a lot of -OH groups (hydrogen bonding). Substance B only contains carbons and hydrogens. Which is more soluble in a polar solvent such as isopropyl alcohol?

A

Like dissolves like.

300
Write an equilibrium expression for the following reaction.


C (s) + H2O (g) > CO(g) + H2(g)

K = [products]/[reactants] 

Only gases and aqueous solutions included.

K = [CO][H2] / [H2O]


400
The volume of an oxygen cylinder is 2.025 L. What is the temperature (in degrees Celsius) of the oxygen cylinder when there are 0.0776 moles of oxygen left in the cylinder at a pressure of 723 torr?


R = 0.08206 L*atm/mol*K

pv=NRT

pv/NR = T

T = ~29.2 degrees Celsius

400
Draw the Lewis structure for CH3NH2.


What intermolecular forces are present?

London dispersion forces (present for all molecules)

Dipole-dipole forces (polar bond between carbon and nitrogen)

Hydrogen bonding (between nitrogen and hydrogen)


400
Calculate the molarity of a 25 dL solution that contains 22.6 g of sodium chloride. 
molarity = moles solute / L solution


moles solute = 22.6 g sodium chloride / 58.44 g (molar mass) = 0.387 moles

L solution = 25 dL / 10 = 2.5 L 

0.387 moles / 2.5 L  = 0.1548 M

400
Given the following reaction:

AB (s) <-> A+ (aq) + B- (aq)

What will happen if you remove B- through the addition of an acid? Which way will the reaction shift?

As products are removed, the system will shift to "make up" for that difference and will produce more products. The system will shift to the right.


500

A sample of hydrogen gas has a volume of 7.49 L at a pressure of 22 atmospheres and a temperature of 305.2 degrees Kelvin. What volume of gaseous water is produced by the following reaction at 398.2 degrees Kelvin and 0.975 atmospheres, if all the hydrogen gas reacts with iron(III) oxide?

Reaction: Fe2O3(s) + 3 H2(g) -> 2 Fe(s) + 3 H2O (g)

R = 0.08206 L*atm/mol*K

Use pv=nRT for H2 to solve for moles (n) of H2

Mole ratio of H2 to H2O to solve for moles of H2O

Use pv=nRT again, but this time you are solving for V of water

V = 221 L

500
Calculate the energy required to cool 3 kg of water from 86 degrees Celsius to 32 degrees Celsius. The specific heat of water is 4.184 J/g*C.


Express your answer in kJ and determine if the process is endothermic or exothermic.

Convert 3 kg to g = 3,000 g

q=MCT -> q=(3000)(4.184)(32-86)


q = -677.2 kJ

Our negative q-value indicates that this process is exothermic.


500
If 42.8 mL of 3.02 M sulfuric acid solution is diluted to a final volume of 360 mL, what is the molarity of the diluted solution?
M1V1 = M2V2

M1V1 / V2 = M2

M2 = 0.359 M



500

In an experiment, gaseous hydroiodic acid dissociates into hydrogen gas and iodine gas. 

hydroiodic acid = 0.704 M 

hydrogen gas = 0.180 M

iodine gas = 0.550 M

Set up an equilibrium expression, determine the value of the equilibrium constant given the concentrations, and interpret the value (are products or reactants favored?). 

K = [H2][I2] / [HI]2

Plug in values.

[0.180][0.550] / [0.704]2

K = 0.200 

K < 1 (reactants are favored)

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