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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
Q

What is Charles’s Law?

A

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

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26
Q

What is Avogadro’s Law?

A

Law that states that the volume of a gas is directly proportional to its amount in moles.

V1/n1=V2/n2

27
Q

What is the ideal gas law with constants?

A

P(atm)•V(L)=n(mol)•R(L•atm/mol•K)•T(K)

28
Q

What are the values of temperature, pressure, and volume at STP?

A

T=273 K
P=1 atm
V=22.4 L

29
Q

How to find density of a gas?

A

d= P(pressure)•M(molar mass)/R(gas constant)•T(temperature)

30
Q

Which values are directly and inversely proportional with density?

A

Molar mass is directly proportional, temperature is inversely proportional

31
Q

What is kinetic molecular theory?

A

A model of an ideal gas as a collection of point particles in constant motion undergoing completely elastic collisions.

32
Q

What three things does kinetic molecular theory state?

A
  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
Q

What is the equation of the root mean square velocity?

A

square root of 3RT/M
R: 8.314 J/mol•K
T: K
M: kg/mol

34
Q

What is diffusion?

A

The process by which gas molecules spread out in response to a concentration gradient

35
Q

What is effusion?

A

The process by which a gas escapes from a container into a vacuum through a small hole.

36
Q

What is graham’s law of effusion?

A

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
Q

What is van der Waals equation?

A

The extrapolation of the ideal gas law that considers the effects of intermolecular forces and particle volume in a non ideal gas.

38
Q

At STP, 1 mol is equal to what?

A

22.4 L

39
Q

At STP, how does density relate to molar mass.

A

The density of a gas at STP is proportional to its molar mass.

40
Q

What is thermochemistry?

A

The study of the relationship between chemistry and energy

41
Q

What is energy?

A

The capacity to do work.

42
Q

What is work?

A

The action of a force through a distance.

Pushing a box across the floor

43
Q

What is heat (q)?

A

The flow of energy caused by a temperature difference.

44
Q

What is kinetic energy?

A

The energy associated with the motion of an object.

45
Q

What is thermal energy?

A

A type of kinetic energy associated with the temperature of an object

46
Q

What is potential energy?

A

The energy associated with the position or composition of an object.

47
Q

What is chemical energy?

A

The energy associated with the relative positions of electrons and nuclei in atoms and molecules.

48
Q

Kinetic energy formula and constants?

A

KE=1/2•m(kg)•v^2(m/s)

49
Q

What is the SI unit of energy?

A 
The Joule (J) 
1 J = kg • m^2/s^2
50
Q

What is delta E?

A

The internal energy change of the system

51
Q

What does a negative delta E mean?

A

Energy is leaving the system through heat or work

52
Q

What is thermal equilibrium?

A

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
Q

What is heat capacity (C)?

A

A measure of the systems ability to absorb thermal energy without undergoing a large change in temperature.

54
Q

What is specific heat capacity?

A

The amount of heat required to raise the temperature of 1 g if a substance by 1 C

55
Q

What is the pressure-volume work formula?

A

W = -P • delta V

56
Q

What is an endothermic reaction?

A

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
Q

What is an exothermic reaction?

A

Negative delta H, heat flows out of system

Combustion of natural gas emits heat into surroundings

Warm to the touch

58
Q

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

a. Endothermic
b. Exothermic
c. Exothermic

59
Q

What is enthalpy?

A

The sum of the internal energy of a system and the product of its pressure and volume.

60
Q

Steps of coffee cup calorimetry

A

q(soln) = m(soln) • C(soln) • Delta T
q(rxn) = -q(soln)
Delta H(rxn) = q(rxn)/mol

61
Q

Standard enthalpies of formation formula?

A

Sum of products heat multiplied by their coefficients minus sum of reactants heat multiplied by their coefficients.

62
Q

What are the units of v = c/lambda

A

Frequency = speed of light/wavelength

63
Q

Energy formula using wavelength?

A

E = h(planck’s constant)•c(speed of light)/wavelength

64
Q

Number of photons?

A

E(pulse) / E(photon)

Chem 1A (7 decks)

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