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WorksheetsHonors Chem Chapter 9
Total questions: 65
Worksheet time: 5hrs 25mins
Convert the following pressure: 1650 torr to atm.
(a)
Convert the following pressure: 3.50 x 10^5 atm to mmHg.
(a)
Convert the following pressure: 185 mmHg to atm.
(a)
Convert the following pressures: 5.65 kPa to atm.
(a)
Convert the following pressures: 190 mmHg to torr.
(a)
Convert the following pressure: 85.0 mmHg to kPa.
(a)
Convert the following pressure: 20.2 inHg to mmHg.
(a)
Convert the following pressures: 0.025 atm to mmHg.
(a)
Convert 37.0°C to Kelvin.
(a)
Convert -27°C to Kelvin.
(a)
Convert 224K to Celsius.
(a)
Convert 875K to Celsius.
(a)
Convert 62°C to Kelvin.
(a)
Convert 200K to Celsius.
(a)
Convert 25°C to Kelvin.
(a)
Convert 100K to Celsius.
(a)
Convert 145°C to Kelvin.
(a)
1.00 L of a gas at standard temperature and pressure is compressed to 325 mL. What is the new pressure of the gas if the temperature is held constant?
3.08 atm
0.00308 atm
0.325 atm
0.840 atm
840 atm
If a 2.38 mole sample of ethane gas occupies a volume of 2.5 L, what is the new volume if the total ethane sample was brought to 4.51 moles of gas? Assume constant pressure and temperature.
4.74 L
2.05 L
7.25 L
4.58 L
In a thermonuclear device, the pressure of 0.065 liters of gas within the bomb casing reaches 3.2 x 10^6 atm. When the bomb casing is destroyed by the explosion, the gas is released into the atmosphere where it reaches a pressure of 1.00 atm. What is the volume of the gas after the explosion?
4.92 x 10^7 liters
2.08 x 10^5 liters
208 liters
20,800 liters
4.92 x 10^4 liters
The temperature inside a refrigerator is about 4.0° Celsius. If a balloon is placed in the fridge that initially has a temperature of 28°C and a volume of 0.78 liters, what will be the volume of the balloon when it is fully cooled by the refrigerator?
0.28 liters
0.31 liters
0.72 liters
It remains the same
0.85 liters
Your brother heats a balloon in the oven. If the balloon initially has a volume of 0.40 liters and a temperature of 20 °C, what will the volume of the balloon be after he heats it to a temperature of 250 °C?
0.51 liters
0.71 liters
1.0 liters
5.0 liters
Your sister blows up a balloon half-way. There are currently 0.85 moles of gas in the balloon and it occupies 1.25 L. If your sister blows more air into the balloon until it has a volume of 2.12 L. What is the new total of moles of gas in the balloon?
1.4 moles
3.1 moles
0.50 moles
1.8 moles
4.8 moles
If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?
29.57 liters
17.64 liters
19.71 liters
21.86 liters
A gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299 K. If I raise the temperature to 350 K and lower the pressure to 1.5 atm, what is the new volume of the gas?
61 liters
31 liters
41 liters
51 liters
21 liters
What volume will 25.0 g of neon occupy at STP?
27.8 L
560 L
11.3 L
5.6 L
319 L
What volume will 0.0591 moles of gas occupy at a temperature of 25.0 °C and a pressure of 0.250 atm
5.78 L
0.485 L
2.52 L
3.06 L
0.291 L
What is the pressure of a 0.0971 mole sample of gas in a 0.750 L container at 25°C?
3.17 atm
3.88 atm
2.45 atm
2.59 atm
1.22 atm
If 5.00 moles of a gas are at a pressure of 7.6 atm and a volume of 12 liters, what is the temperature of the gas?
222 K
273 K
333 K
285 K
156 K
How many moles of gas are present at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 °C?
0.5 moles
1.3 moles
2.5 moles
3.2 moles
1.9 moles
3.16 moles of gas are in a container with a volume of 60.0 liters and at a temperature of 400 K, what is the pressure of the gas in kPa inside the container?
1.73 kPa
175 kPa
1310 kPa
225 kPa
1.38 kPa
If 7.7 moles of gas are at a pressure of 96.24 kPa and at a temperature of 250K, what is the volume of the container that the gas is in?
150 L
218 L
166 L
306 L
143 L
If 17.0 moles of gas are at a temperature of 67 °C, and a volume of 88.89 liters, what is the pressure of the gas in torr?
5.34 torr
4057 torr
1.052 torr
0.007026 torr
540.1 torr
Calculate the density of carbon dioxide gas in grams per liter at 2.00 atm and 0°C.
1.80 g/L
3.93 g/L
2.00 g/L
2.20 g/L
4.12 g/L
Calculate the density of gas A (molar mass 73.0 g/mol) in grams per liter at 1216 torr atm and 300 K.
3604 g/L
4.74 g/L
2500 g/L
2.31 g/L
4.12 g/L
When 2.40 grams of a certain volatile liquid are heated, the volume of the resulting vapor is 821 mL at a temperature of 127°C at standard pressure. What is the molar mass of this substance?
30.5 g/mol
96.0 g/mol
0.0960 g/mol
0.0305 g/mol
14.8 g/mol
A 50.0 gram sample of an ideal gas occupies a volume of 3.2 liters at 40°C and exerts a pressure of 2.6 atm. What is its molar mass?
1043 g/mol
1581 g/mol
154.4 g/mol
19.74 g/mol
133.4 g/mol
How many grams of methane (CH₄) are present at a pressure of 0.60 atm, a volume of 12.5 L, and a temperature of 92°C?
Molar mass of methane is 16.04 g/mol
5.6 grams
4.01 grams
16.04 grams
0.250 grams
2.19 grams
Calculate the density of neon gas in grams per liter at 1.5 atm and -15°C.
24.6 g/L
1.43 g/L
95.1 g/L
-5530 g/L
3.17 g/L
How many grams of ethane (C₂H₆) are present at a pressure of 95.0 kPa, a volume of 9.8 liters, and a temperature of 114 °C?
The molar mass of C2H6 = 30.1 g/mol
882 grams
8.71 grams
16.8 grams
22.4 grams
716 grams
Calcium carbonate decomposes at high temperatures to form carbon dioxide and calcium oxide: CaCO₃(s) → CO₂(g) + CaO(s)
How many grams of calcium carbonate will I need to form 3.45 liters of carbon dioxide at 1.00 atm and 298K?
3.5 grams
5.0 grams
14.1 grams
9.0 grams
10.5 grams
Automobile air bags are inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN₃: 2 NaN₃(s) → 2 Na(s) + 3 N₂(g) If an airbag has a volume of 45 L, and is to be filled with nitrogen gas at 1.05 atm and 28°C, how many grams of NaN₃ must be decomposed?
65.31 grams
82.88 grams
100.5 grams
116.7 grams
24.45 grams
When chlorine is added to acetylene, 1,1,2,2-tetrachloroethane is formed:
C₂H₂(g) + 2 Cl₂(g) → C₂H₂Cl₄(l)
How many liters of chlorine will be needed to make 75.0 grams of C₂H₂Cl₄ at 1.00 atm and 298K?
Molar mass of C2H2Cl4 = 167.8 g/mol
22.4 liters
21.9 liters
67.2 liters
89.6 liters
17.8 liters
Oxygen gas can be prepared in the laboratory by decomposition of potassium nitrate according to the equation:
2 KNO₃(s) → 2 KNO₂(s) + O₂(g)
What mass of KNO₃ forms along with 12.5 L of O₂ measured at 1275 torr and 300K?
0.852 grams
1.67 grams
101 grams
202 grams
71.0 grams
Sulfuric acid, H₂SO₄, decomposes into solid sulfur, water, and oxygen gas according to this chemical equation:
2 H₂SO₄(aq) → 2 S(s) + 3 O₂(g) + 2 H₂O(l)
If 1.56 moles of H₂SO₄ decomposed at 355°C, 1.45 atm, what volume of oxygen was produced?
22.4 liters
83.2 liters
44.8 liters
56.0 liters
71.3 liters
When a hydrochloric acid (HCl) is poured over solid iron, hydrogen gas is produced according to this equation:
Fe(s) + 2 HCl(aq) → H₂(g) + FeCl₂(aq)
If 625 mL of 1.75M HCl is poured over a large bar of solid Fe, what volume of H₂ gas is formed at 310K and 1650 torr?
6.41 L
12.3 L
24.5 L
37.5 L
0.816 L
Our body digests glucose according to this balanced chemical reaction:
C₆H₁₂O₆(s) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O(l)
What volume of CO₂ is produced from the digestion of 125 grams of glucose? Your body temperature is 37°C, and atmospheric pressure in Tucson is 0.91 atm.
The molar mass of glucose, C6H12O6, = 180.2 g/mol
116 liters
44.8 liters
67.2 liters
218 liters
180 liters
He and Ar are both noble gases, are nonpolar, and experience only London dispersion forces (LDF's). Which one has the higher boiling point and why?
He has more electrons and is therefore more polarizable.
He has fewer electrons and is therefore not as polarizable.
Ar has more electrons and is therefore more polarizable.
Ar has fewer electrons and is therefore not as polarizable.
Methane is CH4, and carbon tetrachloride is CCl4. They are both nonpolar and therefore only experience London dispersion forces (LDF's). Which one has the higher boiling point and why?
CH4 because it has more electrons and is therefore more polarizable.
CH4 because it has fewer electrons and is therefore not as polarizable.
CCl4 because it has more electrons and is therefore more polarizable.
CCl4 because it has fewer electrons and is therefore not as polarizable.
Which statement explains why Cl2 is a gas and Br2 is a liquid at 25 °C and 1 atm?
Cl2 has a higher molecular weight than Br2, making it a gas.
Br2 has stronger intermolecular forces than Cl2, making it a liquid.
Cl2 is more reactive than Br2, which determines its state.
Br2 has a lower boiling point than Cl2.
Explain why H2 is a gas and I2 is a solid at 25 °C and 1 atm.
Because of their molecular structures and electronegativities
Due to their positions in the periodic table.
Because of their atomic masses.
Due to the difference in their electron configurations.
I2 has more electrons than H2 and therefore experiences stronger IMF's, keeping it a solid at room temperature.
Which of the following best explains why propane, C3H8, melts at -306.4 °F and decane, C10H22, melts at 345.4 °F?
Propane has a higher molecular weight than decane.
Decane has more electrons than propane, leading to stronger London dispersion forces.
Propane is a gas at room temperature, while decane is a liquid.
Decane has a lower boiling point than propane.
The structures for ethanal, C2H4O, and methanol, CH3OH, are shown. Identify the types of IMF's that exist in pure samples of each.
Ethanal experiences (a)
Methanol experiences (b)
Which gas is more soluble in water: Ne(g) or CO(g) and why?
Ne(g) because it is polar
CO(g) because it is polar
CO(g) because it is nonpolar
Ne(g) because it is nonpolar
They are both equally soluble in water because they are both polar
Which one of the following has the highest boiling point?
CH4
C2H6
C3H8
C4H10
C5H12
The picture shows two completely identical mason jars. They're both filled with the same gas, only one of them has more in it (more molecules). What can you say about the pressures of both jars?
P1 > P2 (greater pressure in jar 1)
P1< P2 (greater pressure in jar 2)
P1 = P2 (same pressure in both)
There's not enough info to tell
Which container will have lower pressure?
First container
second container
A 500 mL gas at 2 atm pressure is compressed to 250 mL. What is the new pressure of the gas?
1 atm
2 atm
4 atm
8 atm
Given a constant temperature, if you start with a gas at 100 kPa and 50 L, and then compress the gas to 25 L, what will be the new pressure?
50 kPa
100 kPa
200 kPa
400 kPa
If a gas at 120 kPa of pressure is expanded from 1 L to 2 L, what is the final pressure of the gas?
60 kPa
120 kPa
240 kPa
480 kPa
If the volume of a gas is decreased from 4.0 L to 2.0 L while keeping the temperature constant, how does the pressure change?
The pressure decreases by half.
The pressure remains the same.
The pressure doubles.
The pressure increases by four times.
With Boyles Law, ____________ is constant.
With Charles law, what is constant?
According to Charles Law, if the temperature is doubled while the volume remains constant, what happens to the pressure?
Arrange the following in order of increasing boiling point?
(start with the substance with the lowest boiling point and increase from there)
H2
CO
H2O
