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Chem 1A > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

What is the majority component and what is the minority component of solvent and solute?

A

Solvent - majority component

Solute - minority component

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2
Q

What is the solvent in an aqueous solution?

A

Water

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3
Q

What is Molarity (M)?

A

Amount of solute (in mol)
————————————
Volume of solution (in L)

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4
Q

How many moles of NaCl are in 3.2 L of a 0.500 M NaCl solution?

A

Moles NaCl = (3.2 L)(0.500 M) = 1.6 mol

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5
Q

What is a dilute solution?

A

A solution that contains a small amount of solute relative to the solvent

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6
Q

What is a concentrated solution?

A

A solution that contains a large amount of solute relative to the amount of solvent

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7
Q

Is molarity a ratio of solute per liter of solution or per liter of solvent?

A

Solution

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8
Q

You are given the mass of KBr and the volume of a solution. How do you find the molarity?

A

Convert g KBr to mol, divide it by the volume using molarity formula.

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9
Q

How many grams of sucrose are in 1.55 L of 0.758 M sucrose solution?

A

(1.55 L)(0.758 M)=mol • grams sucrose

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10
Q

To what volume should you dilute 0.200 L of a 15.0 M NaOH solution to obtain a 3.00 M NaOH solution?

What formula?

A

M1V1=M2V2

V2=M1V1/M2

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11
Q

What volume (in mL) of a 0.150 M HNO3 solution will completely react with 35.7 mL of a 0.108 M Na2CO3 solution?

A

mL Na2CO3 (mL/1000 L) > L Na2CO3 (L Na2CO3•M Na2CO3) > mol Na2CO3 > mol HNO3 > L HNO3 > mL HNO3

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12
Q

2 A(aq) + B(aq) -> C(aq)

What is the limiting reactant if we mix equal volumes of a 1 M solution of A and 1 M solution of B?

A

A is limiting reactant. Reaction requires 2 mol A for every 1 mol B. B is excess.

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13
Q

What is an acid-base reaction?

A

A reaction in which an acid reacts with a base and the two neutralize each other, producing water.

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14
Q

What is a gas-evolution reaction?

A

A reaction in which two aqueous solutions are mixed and a gas forms, resulting in bubbling.

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15
Q

How do antacids help with heartburn?

A

Antacids work to neutralize the stomach acids and relieve heartburn through acid-base reactions.

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16
Q

Which substance produces H+ ions and which substance produces OH- ions?

A

Acids produce H+ ions in aqueous solutions while bases produce OH- ions in aqueous solutions.

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17
Q

Acid-base reactions involving a strong acid yield what?

A

Water and an aqueous solution

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18
Q

Acid-base reactions involving a weak acid yield what?

A

Water and a salt

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19
Q

If 126 mL of a 1.3 M glucose solution is diluted to 450.0 mL, what is the molarity of the diluted solution?

How do you approach this problem?

A

M1V1=M2V2

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20
Q

Difference between a strong and weak acid?

A

A strong acid completely ionizes in solution. A weak acid does not completely ionize in water.

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21
Q

What is the formula for gas pressure?

A

Force
———
Area

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22
Q

What is a manometer?

A

An instrument used to determine the pressure of a gaseous sample, consisting of a liquid filled U shaped tube with one end exposed to the ambient pressure and the other end connected to the sample.

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23
Q

What are the four basic properties of a gas sample?

A

Pressure (P), volume (V), temperature (T), and amount in moles (n)

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24
Q

What is Boyle’s Law?

A

Law that states volume of a gas is inversely proportional to its pressure. As volume increases, pressure decreases.

P1V1=P2V2

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25
What is Charles’s Law?
Law that states that the volume of a gas is directly proportional to its temperature. As volume increases, so does temperature. V1/T1=V2/T2
26
What is Avogadro’s Law?
Law that states that the volume of a gas is directly proportional to its amount in moles. V1/n1=V2/n2
27
What is the ideal gas law with constants?
P(atm)•V(L)=n(mol)•R(L•atm/mol•K)•T(K)
28
What are the values of temperature, pressure, and volume at STP?
T=273 K P=1 atm V=22.4 L
29
How to find density of a gas?
d= P(pressure)•M(molar mass)/R(gas constant)•T(temperature)
30
Which values are directly and inversely proportional with density?
Molar mass is directly proportional, temperature is inversely proportional
31
What is kinetic molecular theory?
A model of an ideal gas as a collection of point particles in constant motion undergoing completely elastic collisions.
32
What three things does kinetic molecular theory state?
1. The size of these particles are negligible small 2. The average kinetic energy of a particle is proportional to the temperature in kelvins 3. The collisions of particles are elastic, energy is transferred and none is lost
33
What is the equation of the root mean square velocity?
*square root of* 3RT/M R: 8.314 J/mol•K T: K M: kg/mol
34
What is diffusion?
The process by which gas molecules spread out in response to a concentration gradient
35
What is effusion?
The process by which a gas escapes from a container into a vacuum through a small hole.
36
What is graham’s law of effusion?
Scientific law that states the ratio of effusion rates of two gases is equal to the square root of the inverse of their molar masses.
37
What is van der Waals equation?
The extrapolation of the ideal gas law that considers the effects of intermolecular forces and particle volume in a non ideal gas.
38
At STP, 1 mol is equal to what?
22.4 L
39
At STP, how does density relate to molar mass.
The density of a gas at STP is proportional to its molar mass.
40
What is thermochemistry?
The study of the relationship between chemistry and energy
41
What is energy?
The capacity to do work.
42
What is work?
The action of a force through a distance. | Pushing a box across the floor
43
What is heat (q)?
The flow of energy caused by a temperature difference.
44
What is kinetic energy?
The energy associated with the motion of an object.
45
What is thermal energy?
A type of kinetic energy associated with the temperature of an object
46
What is potential energy?
The energy associated with the position or composition of an object.
47
What is chemical energy?
The energy associated with the relative positions of electrons and nuclei in atoms and molecules.
48
Kinetic energy formula and constants?
KE=1/2•m(kg)•v^2(m/s)
49
What is the SI unit of energy?
``` The Joule (J) 1 J = kg • m^2/s^2 ```
50
What is delta E?
The internal energy change of the system
51
What does a negative delta E mean?
Energy is leaving the system through heat or work
52
What is thermal equilibrium?
The point at which there is no additional net transfer of heat between a system and it’s surroundings. They are the same temperature.
53
What is heat capacity (C)?
A measure of the systems ability to absorb thermal energy without undergoing a large change in temperature.
54
What is specific heat capacity?
The amount of heat required to raise the temperature of 1 g if a substance by 1 C
55
What is the pressure-volume work formula?
W = -P • delta V
56
What is an endothermic reaction?
Positive delta H, heat flows into system. Cold pack is endothermic because the heat flows into it, cooling the athlete. Endothermic reaction is cold to the touch
57
What is an exothermic reaction?
Negative delta H, heat flows out of system Combustion of natural gas emits heat into surroundings Warm to the touch
58
Identify each as either endothermic or exothermic: a. Sweat evaporating from skin b. Water freezing in a freezer c. Wood burning in a fire
a. Endothermic b. Exothermic c. Exothermic
59
What is enthalpy?
The sum of the internal energy of a system and the product of its pressure and volume.
60
Steps of coffee cup calorimetry
q(soln) = m(soln) • C(soln) • Delta T q(rxn) = -q(soln) Delta H(rxn) = q(rxn)/mol
61
Standard enthalpies of formation formula?
Sum of products heat multiplied by their coefficients minus sum of reactants heat multiplied by their coefficients.
62
What are the units of v = c/lambda
Frequency = speed of light/wavelength
63
Energy formula using wavelength?
E = h(planck’s constant)•c(speed of light)/wavelength
64
Number of photons?
E(pulse) / E(photon)

Chem 1A (7 decks)

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