Gases, Liquids and Solids Flashcards
(81 cards)
1
Q
Identify the following change of state as melting, freezing, sublimation or deposition:
the solid structure of a solid breaks down as a liquid forms.
A
Melting.
2
Q
Identify the following change of state as melting, freezing, sublimation or deposition:
coffee is freeze-dried.
A
Sublimation.
3
Q
Identify the following change of state as melting, freezing, sublimation or deposition:
ice crystals form on a package of frozen corn.
A
Deposition.
4
Q
True or False:
Freezing is an endothermic phase change.
A
False.
Freezing releases heat so it is exothermic.
5
Q
True or False:
Melting is an endothermic phase change.
A
True.
Molecules absorb heat as they change from solid to liquid.
6
Q
True or False:
Vaporization is an exothermic phase change.
A
False.
As a substance moves from liquid to gas it absorbs heat.
7
Q
Identify the following change of state:
water vapor in clouds changes to rain.
A
Condensation.
8
Q
Identify the following change of state:
wet clothes dry on a clothes line.
A
Evaporation.
9
Q
Identify the following change of state:
lava flows into the ocean and steam forms.
A
Boiling.
10
Q
What is the main attractive force between BrF molecules?
A
Dipole-dipole bonds.
11
Q
What is the main attractive force between molecules of Cl2?
A
London dispersion bonds.
12
Q
What is the main attractive force between NF3 particles?
A
Dipole-dipole bonds.
13
Q
What is the main attractive force between molecules of HAt?
A
London dispersion bonds.
14
Q
Identify the strongest attractive force in the following: CH3OH.
A
Hydrogen bonds.
15
Q
Identify the strongest attractive force in the following: CO.
A
Dipole-dipole bonds.
16
Q
Identify the strongest attractive force in the following: CF4.
A
London dispersion forces.
17
Q
Rank the following compounds according to their melting points. Rank from the highest melting point to the lowest melting point.
HCl
NaCl
F2
H2O
A
Highest to lowest:
1) NaCl (ionic)
2) H2O (H bonds)
3) HCl (dipole-dipole)
4) F2 (London dispersion).
18
Q
Rank the following compounds according to their melting points. Rank from the highest melting point to the lowest melting point.
HF
H2O
CH4
H2S
A
Highest to lowert:
1) H20 (H bonds, has 2 H)
2) HF (H bonds)
3) H2S (London dispersion heavier weight)
4) CH4 (London dispersion).
19
Q
Match the property of a gas with its correct measurement.
1) 350 K
2) 10 L
3) 2.00 g O2
4) 755 mmHg
A
1) Temperature
2) Volume
3) Mass
4) Pressure
20
Q
True or False:
The force of the gas particles on the container wall describes the pressure of a gas.
A
True.
21
Q
True or False:
The force/collision of the gas particles on the container wall describes the pressure of a gas.
A
True.
22
Q
True or False:
4.5 L of helium gas describes the pressure of a gas.
A
False.
Liters measures the volume of the gas.
23
Q
True or False:
750 torr describes the pressure of a gas.
A
True.
Torr or mmHg measures pressure of gas.
24
Q
True or False:
The average kinetic energy of gas molecules decreases with increasing temperature.
A
False.
Increasing the temperature will increase the speed of particles!
25
True or False:
Most of the volume occupied by a gas is empty space.
True.
26
An oxygen tank your patient uses for their emphysema has a pressure of 2.0 atm. What is the pressure in torr?
1520 torr.
27
An oxygen tank your patient uses for their emphysema has a pressure of 2.0 atm. What is the pressure in mmHg?
1520 mmHg.
28
A gas is measured at 980 torr. What is the pressure in atm?
1.3 atm.
29
Which measurement represents the smallest value of pressure?
755 torr
785 mm Hg
0.750 atm
22.0 psi
0.750 atm.
30
The barometric pressure given in
the local weather report is reported as in Hg. What is the pressure in mmHg if the weatherman says the current pressure
today is 29.75 in Hg?
755.7 mmHg.
31
A gas with a volume of 4.0 L is in a closed container. Match the resulting change in pressure when the following volume changes occur:
1) The volume is compressed to 2.0 L.
2) Volume expands to 12 L.
1) Pressure increases.
2) Pressure decreases.
32
A 10 L balloon contains helium gas at a pressure of 655 mmHg.
Provide the correct final pressure (mmHg) according to the volume changes of this balloon. (assume no changes in temperature or amount of gas).
1) 20 L
2) 2.5 L
3) 13 800 mL
4) 1250 mL
1) 328 mmHg.
2) 2620 mmHg.
3) 475 mmHg.
4) 5240 mmHg.
33
A sample of nitrogen, N2, has a volume of 50.0 L at a pressure of 760 mmHg.
Provide the correct final volume (L) according to the pressure changes of this balloon. (assume no changes in temperature or amount of gas).
1) 725 mmHg.
2) 2 atm.
3) 0.5 atm.
4) 850 torr.
1) 52.3 L.
2) 25 L.
3) 100 L.
4) 45 L.
34
Cyclopropane,C3H6, is a general anaesthetic. A 5.0 L sample of cyclopropane has a pressure of 5.0 atm. What is the volume, in liters, of the anaesthetic, given to a patient at a pressure of 1.0 atm with no change in temperature or amount of gas?
25 L.
35
Match the terms inspiration and expiration to correctly describe the part of the breathing cycle given:
1) The diaphragm contracts (flattens out).
2) The volume of air in the lungs decreases.
1) Inspiration.
2) Expiration.
36
True or False: During inspiration, the pressure within the lungs is greater than that of the atmosphere.
False.
The pressure in the lungs is less than the pressure in the atmosphere during inspiration.
37
A sample of neon gas has a volume of 2.5 L at 15°C. Match the temperatures, in degrees Celsius, required to obtain the volumes listed below. (Assume n and P do not change).
1) 5 L.
2) 1,250 mL.
3) 7.50 L.
4) 3,550 mL.
1) 303 °C.
2) - 129 °C.
3) 591 °C.
4) 136 °C.
Convert to K first, then convert back.
38
A balloon contains 2500 mL of helium gas at 75°C. Match the following final volumes of helium gas, in mL, with the correct temperature required to obtain each final volume. (Assume n and P do not change).
1) 55 Celsius.
2) 680 K.
3) - 25 Celsius.
4) 240 K.
1) 2400 mL.
2) 4900 mL.
3) 1800 mL.
4) 1700 mL.
39
Charles' Law states...
The volume of a gas is directly proportional to its temperature, in K, when n and P are held constant.
40
What is the final pressure, in torr, of a gas with an initial pressure of 1200 torr at 155°C is cooled to 0°C.
770 torr.
41
What is the final pressure, in torr, of a gas in an aerosol can with an initial pressure of 1.40 atm at 12°C is heated to 35°C.
1150 torr.
42
Calculate the final temperature, in degrees Celsius, if a sample of xenon gas at 25°C and 740 mmHg is cooled to give a pressure of 620 mmHg.
-23°C.
43
Calculate the final temperature, in degrees Celsius, if a tank of argon gas with a pressure of 0.950 atm at -18°C is heated to give a pressure of 1250 torr.
168°C.
44
A sample of helium gas has a volume of 6.50 L at a pressure of 845 mmHg and a temperature of 25°C. What is the final pressure of the gas, in atm, when the volume and temperature of the gas are changed to 1850 mL and 325K?
4.26 atm.
45
A sample of helium gas has a volume of 6.50 L at a pressure of 845 mmHg and a temperature of 25°C. What is the final pressure of the gas, in atm, when the volume and temperature of the gas are changed to 2.25 L and 12°C?
3.07 atm.
46
A sample of helium gas has a volume of 6.50 L at a pressure of 845 mmHg and a temperature of 25°C. What is the final pressure of the gas, in atm, when the volume and temperature of the gas are changed to 12.8 L and 47°C?
0.606 atm.
47
A 124 mL bubble of hot gases at 212°C and 1.80 atm, is emitted from an active volcano. What is the final temperature, in degrees Celsius, of the gas in the bubble outside the volcano if the final volume of the bubble is 138 mL and the pressure is 0.800 atm?
- 33°C.
48
A sample containing 1.50 moles of Ne gas has an initial volume of 8.00 L. What is the final volume of the gas, in liters, when a leak allows one-half of the Ne atoms to escape?
4.00 L.
49
A sample containing 1.50 moles of Ne gas has an initial volume of 8.00 L. What is the final volume of the gas, in liters, when a sample of 3.50 moles of Ne is added to the 1.50 moles of Ne gas in the container?
26.7 L.
50
A sample containing 1.50 moles of Ne gas has an initial volume of 8.00 L. What is the final volume of the gas, in liters, when a sample of 25.0 g of Ne is added to the 1.50 moles of Ne gas in the container?
14.6 L.
51
Using molar volume, calculate the number of moles of O2 in 44.8 L of O2 gas (assume STP).
2.00 mol.
52
Using molar volume, calculate volume, in liters, occupied by 0.420 mole of He gas (assume STP).
9.41 L of He.
53
Using molar volume, calculate the volume, in L, of 6.40 g of O2 gas (assume STP).
4.48 L.
54
Using molar volume, calculate the number of grams of H2 in 1620 mL of H2 gas (assume STP).
0.146 g.
55
Boyle, with much help from his friends developed a law correlating pressure and volume of a gas which states:
Pressure is inversely correlated to volume.
56
The Ideal Gas Law is given by:
PV = nRT.
57
Why does a pop can get crushed when it moved from the hot plate to the ice bath?
Because the atmospheric pressure outside the can was greater than inside the can.
58
What volume will 0.250 mol of O2 (g) occupy at STP?
5.60 L
59
A sample of 4.25 moles of hydrogen at 20.0°C occupied a volume of 25.0 L. What is the pressure, in kPa, of this sample?
414 KPa.
60
What volume will 30.0 g of NO(g) occupy at 3.26 atm and 19.0°C?
7.34 L
61
In a gas mixture, the partial pressures are: nitrogen 425 torr, oxygen 115 torr, and helium 225 torr. What is the total pressure, in torr, of the gas mixture?
765 torr.
62
A gas mixture containing oxygen, nitrogen and helium exerts a total pressure of 925 torr. If the partial pressures are: oxygen 425 torr and helium 75 torr, what is the partial pressure, in torr, of the nitrogen in the mixture?
425 torr.
63
In lung diseases such as emphysema, there is a decrease in the ability of oxygen to diffuse into the blood. How would the partial pressure of oxygen in the person's blood change as a result of having emphysema?
Their partial pressure of oxygen in the blood would decrease.
64
In lung diseases such as emphysema, there is a decrease in the ability of oxygen to diffuse into the blood. Why does a person with severe emphysema sometimes use a portable oxygen tank?
The increased oxygen pressure in the patient's lungs will raise the partial pressure of oxygen in their blood.
65
As the temperature of a liquid is
increased, what happens to its vapor pressure?
Its vapor pressure rises.
66
As the temperature of a liquid is
decreased, what happens to its vapor pressure?
Its vapor pressure drops.
67
Vapor pressure depends on:
Both temperature and chemical identity of the liquid.
68
A solid compound which has no
definite crystalline structure and a poorly defined melting point is referred
to as a(an) ________ solid.
Amorphous.
69
Which type of solid does the following
description best describe?
shiny, ductile; malleable;
conductors of heat and electricity; crystalline.
Alloy.
70
Which type of solid does the following
description best describe?
hard; very high melting point;
crystalline.
The atoms are held together by
covalent bonds in all directions. This combination makes the network very
strong.
Covalent network.
71
Calculate the heat (in cal) change at 0°C for the following and state whether heat was absorbed or released:
calories to melt 65 g of ice
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vaporization (H2O) = 540 cal/g or 2260 J/g
5200 cal, heat absorbed.
72
Calculate the heat change (in J) at 0°C for the following and state whether heat was absorbed or released:
joules to melt 17.0 g of ice
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g
5680 J, absorbed.
73
Calculate the heat change (in kcal) at 0°C for the following and state whether heat was absorbed or released:
kilocalories to freeze 225g of water
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g
18 kcal, released.
74
Calculate the heat change (in kJ) at 0°C for the following and state whether heat was absorbed or released:
kilojoules to freeze 50 g of water
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g
16.7 KJ, released.
75
Calculate the heat change (in cal) at 100°C for each of the following and indicate whether heat is absorbed or released:
calories to vapourize 10.0 g of water
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g
5400 cal, absorbed.
76
Calculate the heat change (in J) at 100°C for each of the following and indicate whether heat is absorbed or released:
joules to vapourize 5 g of water
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g
11300 J, absorbed.
77
Calculate the heat change (in kcal) at 100°C for each of the following and indicate whether heat is absorbed or released:
kilocalories to condense 8.0 kg of steam
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g.
4320 kcal, released.
78
Calculate the heat change (in kJ) at 100°C for each of the following and indicate whether heat is absorbed or released:
kilojoules to condense 175 g of steam
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g.
396 kJ, released.
79
Using the values for heat of fusion (in J), specific heat of water or heat of vapourization, calculate the energy in the following:
joules needed to melt 50.0 g of ice at 0°C and to warm the liquid to 65°C
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vaporization (H2O) = 540 cal/g or 2260 J/g.
30 300 J.
80
Using the values for heat of fusion (in kcal), specific heat of water or heat of vapourization, calculate the energy in the following:
kilocalories released when 15.0 g of steam condenses at 100°C and the liquid cools to 0°C
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g.
9.6 kcal.
81
Using the values for heat of fusion, specific heat of water or heat of vapourization, calculate the energy (in kJ) in the following:
kilojoules needed to melt 24.0 g of ice at 0°C, warm the liquid to 100°C and change it to steam at 100°C
Heat of Fusion (H2O) = 79.7 cal/g or 333 J/g
Heat of Vapourization (H2O) = 540 cal/g or 2260 J/g.
72.3 KJ.
