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Chemistry > Semester Exam > Flashcards

Semester Exam Flashcards

1
Q

a weak electrolyte exists predominantly as — in solution

A

molecules

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2
Q

which are the strongest electrolytes

A

HCl, KCl

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3
Q

The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and CaCl2 are mixed is

A

Ca^2+(aq) + CO3^2- (aq) –> CaCO3 (s)

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4
Q

which of the following are strong acids

A

HI, HNO3, HBr

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5
Q

Aqueous potassium chloride will react with which one of the following in an exchange (metathesis)

A

Lead Nitrate

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6
Q

Which of the following is soluble in water at 25 degrees Celsius

A

Fe(NO3)2

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7
Q

When aqueous solutions of — are mixed, a precipitate forms.

A

NiBr2 and AgNO3

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8
Q

Which one of the following compounds is insoluble in water?

A

ZnS

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9
Q

With which of the following will the ammonium ion form an insoluble salt

A

none of the above

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10
Q

The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is —

A

H+ (aq) + OH^- (aq) —-> H2O (l)

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11
Q

Which of these metals is the least easily oxidized?

A

Au

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12
Q

How many grams of NaOH (MW=40) are there in 500 mL of a 0.175 M NaOH solution>

A

3.50

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13
Q

How many grams of CH3OH must be added to water to prepare 150mL of a solution that is 2.0 M CH3OH

A

9.6

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14
Q

There are— mol of bromide ions in .500 L of a .300 M solution of AlBr3

A

.450

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15
Q

An aqueous ethanol solution (400mL) was diluted to 4L, giving a concentration of 0.0400 . The concentration of the original solution was —– M

A

.400 M

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16
Q

The molarity (M) of an aqueous solution containing 22.5g of glucose (C6H12O6) in 35.5 mL of solution is

A

3.52

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17
Q

In a titration of 35mL of 0.737 M H2SO4 — mL of a 0.827 M KOH solution is required for neutralization

A

62.4

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18
Q

In which species does nitrate have the highest oxidation number?

A

NaNO3

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19
Q

OF the choices below, which would be the best for the lining of a tank intended for use in storage of hydrochloric acid?

A

Copper

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20
Q

Oxidation is the — and reduction is the —-

A

loss or electrons, gain of electrons.

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21
Q

Calculate the kinetic energy in J of an electron moving at 6.00x10^6 m/s. The mass of an electron is 9.11x10^-28g

A

1.64x10^-17

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22
Q

The kinetic energy of a 23.2-g object moving at a speed of 81.9m/s is —– J.

A

77.8 J

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23
Q

A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample increases from 23.2degreesC to 30.5degreesC. Since the specific heat capacity of aluminum is 0.90J/g-K, the mass of the sample is —–g

A

1.5 g

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24
Q

At what velocity (m/s) must a 20.0g object be moving in order to posses a kinetic energy of 1.00J?

A

10.0

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25
Q

The units of heat capacity are

A

J/K or J/degreesC

26
Q

22.44g samples of iron absorbs 180.8J of heat, upon which the temperature of the sample increases from 21.1degreesC to 39.0degreesC. What is the specific heat of iron?

A

0.450

27
Q

Given the following reactions
1). 2NO–>N2 +O2 deltaH= 44.01kJ
2). 2NO+O2–>2NO2 deltaH= -112kJ
the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide
N2+2O2–>2No2

A

68kJ

28
Q

Given the following reactions
H2O(l) –> H2O(g) deltaH= 44.01kJ
2H2(g)+O2(g)–>2H2O(g) deltaH= -483.64kJ
the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen
2H2O(l)–>2H2(g)+O2(g)

A

571.66kJ

29
Q

Given the data in the table below, deltaH degree-rxn for the reaction 4NH3(g)+5O2(g)–>4NO(g)+6H2O(l)
*Table

A

-1172

30
Q

Given the data in the table below, deltaHdegrees-rxn for the reaction C2H5OH(l)+O2(g)–>CH3CO2H(l)+H2O(l)
*Tab;e

A

-492.6

31
Q

THe wavelength of light emitted from a traffic light having a frequency of 5.75x10^14Hz is

A

521nm

32
Q

The uncertainty principle states that

A

it is impossible to know the exact position and momentum of an electron

33
Q

Which of the following is an incorrect subshell notation

A

2d

34
Q

Which set of thee quantum number (n,l,ml) corresponds to a 3d orbital

A

3,2,2

35
Q

Ifa n electron has a principle quantum number (n) of 3 and an azimuthal quantum number (l) of 2, the subshell designation is

A

3d

36
Q

Which of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranged as n,l,ml, and ms)

A

1,0,0,1/2

37
Q

The ground state electron configuration of Fe is

A

1s^2, 2s^2,2p^6,3s^2,3P^63d^64s^2

38
Q

Electromagnetic radiation with a wavelength of 525nm appears as green light to human eyeThe frequency is–

A

5.71x10^14

39
Q

The element that corresponds to the electron configuration 1s^2,2s^2,2p^6 is

A

neon

40
Q

The condensed electron configuration of krypton, element 36, is

A

[Ar]3d^10,4s^2,4p^6

41
Q

a sample of gas (5.0mol) at 1.0atm is expanded at constant temperature from 10L to 15L. The final pressure is

A

.67atm

42
Q

If 50.75g of gas occupies 10L at STP, 129.3g of the gas will occupy

A

25.5 at STP

43
Q

The presage of a sample of CH4 gas (6.022) in a 30L vessel at 402K is

A

0.413

44
Q

The pressure exerted by 1.3 mol of gas in a 13L flask at 22degreesC and 2.5atm and—

A

250kPa

45
Q

A sample of gas (1.3mol) occupies –L at 22degreesC and 2.5atm

A

13

46
Q

The density of ammonia gas in a 4.32L container at 837torr and 45degreeC is

A

.719 g/L

47
Q

Automobile airbags use the decomposition of sodium azide as their source of gas for rapid inflation
2NaN3–>2Na+ 3N2
what mass of 2NaN3 is required to provide 40L of N2 at 25degreesC and 763torr

A

71.1g

48
Q

A vessel contained N2, Ar,He, and Ne. The total pressure in the vessel was 987 torr. The partial pressure of nitrogen, argon, and helium were 44, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was

A

239 torr

49
Q

Which of the following equations shows an incorrect relationship between pressures given in terms of different units?

A

1.0 torr = 2.00mm Hg

50
Q

The molar volume of a gas at STP is

A

22.4 L

51
Q

Of the following substances, only—- Has London Dispersion forces as its inly intermolecular forces

A

CH4

52
Q

Of the following,— has the highest boiling point. (Graph)

A

Br2

53
Q

The heating curve shown was generated by measuring the heat flow and temperature of a solid as it was heated. The heat flow into the sample in the segment—- will yield the value of the deltaH of this substance

A

DE

54
Q

The normal boiling point of the substance with the phase diagram shown above is

A

40degreesC

55
Q

Which statement is true about liquids but not true about solids

A

They flow and are not compressible

56
Q

What is the predominate intermolecular force in Cbr4

A

London-Dispersions

57
Q

Which statements about viscosity are true

A

all

58
Q

The vapor pressure of a liquid

A

increases nonlinearly with temperature.

59
Q

Calculate the freezing point (0degreesC) of a 0.05500m aqueous solution of glucose. The molal freezing-point-depression constant of water is 1.86

A

-0.102

60
Q

A solution with a concentration higher than the solubility is

A

a supersaturated

Chemistry (1 decks)

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