Question 1

What is the Celsius temperature of 100.0 g of chlorine gas in a 40.0-L container at 800 mm Hg?
A)-91°C
B)91°C
C)182°C
D)364°C

Accepted Answer

The correct answer is B.The ideal gas law can be used to calculate the temperature of the chlorine gas. The ideal gas law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.We can rearrange the ideal gas law to solve for T: T = PV/nR.We know the pressure, volume, and number of moles of chlorine gas. We can look up the value of the ideal gas constant, which is 0.0821 L*atm/(mol*K).Plugging in our values, we get: T = (800 mm Hg * 1 atm/760 mm Hg) * 40.0 L / (100.0 g * 1 mol/70.9 g/mol) * 0.0821 L*atm/(mol*K) = 364 K.Converting to Celsius, we get: T = 364 K - 273.15 = 91°C.

Question 2

A basketball is inflated to a pressure of 1.50 atm in a 20.0°C garage.What is the pressure of the basketball outside where the temperature is -5.00°C?
A)1)37 atm
B)1)42 atm
C)1)58 atm
D)1)64 atm

Accepted Answer

According to Charles's law, the pressure of a gas is directly proportional to its temperature. Therefore, as the temperature of the basketball decreases, its pressure will also decrease. The correct answer is A) 1.37 atm.

Question 3

Cyanogen is a gas which contains 46.2% C and 53.8% N by mass.At a temperature of 25°C and a pressure of 750 mm Hg,1.50 g of cyanogen occupies 0.714 L.What is the molecular formula of cyanogen? A)CN B)C₂N₂ C)C₃N₄ D)C₄N₅

Accepted Answer

The answer of Cyanogen is a gas which contains 46.2%...

Question 4

The volume of 350.mL of gas at 25°C is decreased to 125 mL at constant pressure.What is the final temperature of the gas?
A)-167°C
B)8)9°C
C)70°C
D)561°C

Accepted Answer

According to Charles's law, if the pressure is constant, the volume of a gas is directly proportional to its temperature, so V1/T1=V2/T2. Solving for T2, T2= (V2 x T1)/V1. Plugging in the values, we get T2= (125 mL x 298 K)/350 mL = 106.9 K. Converting to Celsius, T2= -166.1°C, which rounds to -167°C. Therefore, the correct answer is A).

Question 5

A gas occupies 22.4 L at STP and 14.5 L at 100°C and 2.00 atm pressure.How many moles of gas did the system gain or lose?
A)0)06 moles gained
B)0)03 moles gained
C)0)03 moles lost
D)0)05 moles lost

Accepted Answer

The answer of A gas occupies 22.4 L at STP...

Question 6

A 1.75 L container filled with CO₂ gas at 25°C and 225 kPa pressure springs a leak.When the container is re-sealed,the pressure is 185 kPA and the temperature is 10°C.How many moles of gas were lost? A)0)0213 mol B)0)463 mol C)0)561 mol D)2)16 mol

Accepted Answer

The answer of A 1.75 L container filled with CO₂...

Question 7

A balloon filled with helium gas at 20°C occupies 2.91 L at 1.00 atm.The balloon is immersed in liquid nitrogen at -196°C,raising the pressure to 5.20 atm.What is the volume of the balloon in the liquid nitrogen?
A)0)15 L
B)2)1 L
C)4)0 L
D)58 L

Accepted Answer

We can use the combined gas law to solve for the volume of the balloon in liquid nitrogen:

(P₁V₁/T₁) = (P₂V₂/T₂)

Where:
P₁ = 1.00 atm
V₁ = 2.91 L
T₁ = 20°C + 273.15 = 293.15 K
P₂ = 5.20 atm
V₂ = Unknown (what we are solving for)
T₂ = -196°C + 273.15 = 77.15 K

Solving for V₂:

V₂ = (P₁V₁T₂)/(P₂T₁)
V₂ = (1.00 atm)(2.91 L)(77.15 K)/((5.20 atm)(293.15 K))
V₂ = 0.15 L

Therefore, the volume of the balloon in liquid nitrogen is 0.15 L. The best choice is A).

Question 8

If the number of moles of gas is doubled at constant temperature and volume,the pressure of the gas
A)is halved.
B)is doubled.
C)is quadrupled.
D)remains the same.

Accepted Answer

According to the ideal gas law, PV=nRT, pressure (P), volume (V), and temperature (T) are directly proportional to the number of moles of gas (n). As the number of moles of gas is doubled at constant temperature and volume, both P and V would double to maintain the equality of the equation. So, the pressure of the gas would also double.

Question 9

A 1.00 L flask contains nitrogen gas at 25°C and 1.00 atm pressure.What is the final pressure in the flask if an additional 2.00 g of N₂ gas is added to the flask and the flask cooled to -55°C? A)1)28 atm B)2)01 atm C)2)56 atm D)3)29 atm

Accepted Answer

The answer of A 1.00 L flask contains nitrogen gas...

Question 10

A steel bottle contains argon gas at STP.What is the final pressure if the temperature is changed to 115°C?
A)0)704 atm
B)0)768 atm
C)1)30 atm
D)1)42 atm

Accepted Answer

According to the Ideal Gas Law, PV=nRT, if the number of moles of gas and the volume of the container remains constant, then the pressure and temperature are directly proportional. As the temperature increases from 273 K (STP) to 388 K (115°C or 115+273), the pressure will also increase in proportion. Using the formula P1/T1=P2/T2 and substituting the values, we get P2 = (P1*T2)/T1 = (1 atm * 388 K)/273 K = 1.42 atm. Therefore, the final pressure is 1.42 atm or approximately 1.4 atm. The correct choice is D).

Question 11

How many grams of O₂ gas are there in a 5.00-L cylinder at 4.00 × 10³ mm Hg and 23°C? A)17.3 g B)34.7 g C)446 g D)2)63 × 10⁴ g

Accepted Answer

We can use the Ideal Gas Law equation: PV = nRT P = 4.00 × 10^13 mm Hg (convert to atm by dividing by 760 mm Hg/atm) = 5.26 x 10^9 atm V = 5.00 L T = 23°C + 273.15 = 296.15 K R is the gas constant and n is the number of moles of gas. We need to find n and convert it to grams using the molar mass of O₂ gas. To find n, we rearrange the Ideal Gas Law equation: n = PV/RT n = (5.26 x 10^9 atm)(5.00 L)/(0.0821 L*atm/K*mol)(296.15 K) = 107.8 mol The molar mass of O₂ gas is approximately 322 g/mol. So, the mass of 107.8 mol of O₂ gas is (107.8 mol)(322 g/mol) = 34,776 g = 34.8 kg. To convert to grams, we multiply by 1000: 34.8 kg x 1000 g/kg = 34,800 g = 34.7 g (to three significant figures). Therefore, the answer is B: 34.7 g.

Question 12

How many molecules of N₂ are in a 500.0 mL container at 780 mm Hg and 135°C? A)8)76 × 10²¹ B)9)23 × 10²¹ C)2)65 × 10²² D)2)79 × 10²²

Accepted Answer

The answer of How many molecules of N₂ are in...

Question 13

A 75.0 L steel tank at 20.0°C contains acetylene gas,C₂H₂,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank? A)4)33 g B)6)01 g C)113 g D)1650 g

Accepted Answer

First, we need to convert the pressure from atm to Pa:

1.39 atm x 101325 Pa/atm = 140236 Pa

Using the Ideal Gas Law equation, we can calculate the number of moles of acetylene in the tank:

PV = nRT

n = (PV) / (RT)

n = (140236 Pa)(75.0 L) / [(8.31 J/mol*K)(293 K)]

n = 4.05 mol

Finally, we can convert moles to grams using the molar mass of acetylene:

4.05 mol x 26.04 g/mol = 105.02 g, rounded to 113 g.

Question 14

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains CH₄,flask B contains CO₂,flask C contains N₂.Which flask contains the largest number of molecules? A)flask A B)flask B C)flask C D)All flasks contain the same number of molecules.

Accepted Answer

The ideal gas law, PV = nRT, can be rearranged to solve for the number of molecules (or moles) present:

n = PV/RT

Since all three flasks are at the same temperature (standard temperature) and pressure (standard pressure), the equation simplifies to:

n = V/22.4

where V is the volume of each flask in liters.

Since all three flasks are identical, they have the same volume. Therefore, they contain the same number of molecules, and the answer is D, "All flasks contain the same number of molecules."

Question 15

"Equal volumes of different gases at the same temperature and pressure contain the same molar amounts" is another way of stating
A)Avogadro's law.
B)Boyle's law.
C)Charles' law.
D)Graham's law.

Accepted Answer

The statement describes Avogadro's law, which states that equal volumes of gases at the same temperature and pressure contain the same number of molecules (or molar amounts) regardless of their chemical composition.

Question 16

What is the value of the gas constant,R,in units of ? A)1)080 × 10^-4 B)0)1080 C)62.36 D)6)236 × 10⁴

Accepted Answer

The value of the gas constant, R, is approximately 8.314 J/(mol·K). Converting this to the given units of TB4939, we get R = 8.314/(10^14*10^-9) TB4939. Simplifying this, we get R = 6.236 × 10^10 TB4939 or R = 6.236 × 10^-4 (in scientific notation). Therefore, the answer is option D, 6.236 × 10^-4.

Question 17

An "empty" aerosol can at 25°C still contains gas at 1.00 atmosphere pressure.If an "empty" can is thrown into a 475°C fire,what is the final pressure in the heated can? A)5)26 × 10^-2 atm B)0)398 atm C)2)51 atm D)19.0 atm

Accepted Answer

Using the ideal gas law, the pressure can be calculated using the formula P1/T1 = P2/T2. Converting temperatures to Kelvin: T1 = 25°C + 273 = 298 K, T2 = 475°C + 273 = 748 K. Solving for P2 gives P2 = (1 atm * 748 K) / 298 K = 2.51 atm.

Question 18

A 0.286-g sample of gas occupies 125 mL at 60.cm of Hg and 25°C.What is the molar mass of the gas?
A)5)9 g/mol
B)44 g/mol
C)59 g/mol
D)71 g/mol

Accepted Answer

The answer of A 0.286-g sample of gas occupies 125...

Question 19

A gas bottle contains 0.650 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?
A)0)0680 mol
B)0)128 mol
C)0)717 mol
D)0)778 mol

Accepted Answer

To find the moles of gas added, use the ideal gas law relation: P1/n1 = P2/n2. Convert 730 mm Hg to atm (730 mm Hg = 0.9605 atm). Then, solve for n2 using P2 = 1.15 atm. The difference n2 - n1 gives the moles added.

Question 20

What is the volume of 10.0 g of argon gas at 157°C and 2.50 kPa pressure?
A)1)29 L
B)3)53 L
C)131 L
D)358 L

Accepted Answer

We can use the ideal gas law to solve for the volume of argon gas:
PV = nRT
n = m/M (where n is the number of moles, m is the mass, M is the molar mass)
V = (m/M)RT/P
V = (10.0 g / 39.95 g/mol) * 8.31 J/mol*K * (157 + 273)K / 2.50 kPa
V = 358 L. Therefore, the correct answer is choice D, 358 L.

Quiz 9: Gases: Their Properties and Behavior

What is the Celsius temperature of 100.0 g of chlorine gas in a 40.0-L container at 800 mm Hg?

A basketball is inflated to a pressure of 1.50 atm in a 20.0°C garage.What is the pressure of the basketball outside where the temperature is -5.00°C?

Cyanogen is a gas which contains 46.2% C and 53.8% N by mass.At a temperature of 25°C and a pressure of 750 mm Hg,1.50 g of cyanogen occupies 0.714 L.What is the molecular formula of cyanogen?

The volume of 350.mL of gas at 25°C is decreased to 125 mL at constant pressure.What is the final temperature of the gas?

A gas occupies 22.4 L at STP and 14.5 L at 100°C and 2.00 atm pressure.How many moles of gas did the system gain or lose?

A 1.75 L container filled with CO2 gas at 25°C and 225 kPa pressure springs a leak.When the container is re-sealed,the pressure is 185 kPA and the temperature is 10°C.How many moles of gas were lost?

A balloon filled with helium gas at 20°C occupies 2.91 L at 1.00 atm.The balloon is immersed in liquid nitrogen at -196°C,raising the pressure to 5.20 atm.What is the volume of the balloon in the liquid nitrogen?

If the number of moles of gas is doubled at constant temperature and volume,the pressure of the gas

A 1.00 L flask contains nitrogen gas at 25°C and 1.00 atm pressure.What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?

A steel bottle contains argon gas at STP.What is the final pressure if the temperature is changed to 115°C?

How many grams of O2 gas are there in a 5.00-L cylinder at 4.00 × 103 mm Hg and 23°C?

How many molecules of N2 are in a 500.0 mL container at 780 mm Hg and 135°C?

A 75.0 L steel tank at 20.0°C contains acetylene gas,C2H2,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank?

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains CH4,flask B contains CO2,flask C contains N2.Which flask contains the largest number of molecules?

"Equal volumes of different gases at the same temperature and pressure contain the same molar amounts" is another way of stating

What is the value of the gas constant,R,in units of ?

An "empty" aerosol can at 25°C still contains gas at 1.00 atmosphere pressure.If an "empty" can is thrown into a 475°C fire,what is the final pressure in the heated can?

A 0.286-g sample of gas occupies 125 mL at 60.cm of Hg and 25°C.What is the molar mass of the gas?

A gas bottle contains 0.650 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?

What is the volume of 10.0 g of argon gas at 157°C and 2.50 kPa pressure?

A 1.75 L container filled with CO₂ gas at 25°C and 225 kPa pressure springs a leak.When the container is re-sealed,the pressure is 185 kPA and the temperature is 10°C.How many moles of gas were lost?

A 1.00 L flask contains nitrogen gas at 25°C and 1.00 atm pressure.What is the final pressure in the flask if an additional 2.00 g of N₂ gas is added to the flask and the flask cooled to -55°C?

How many grams of O₂ gas are there in a 5.00-L cylinder at 4.00 × 10³ mm Hg and 23°C?

How many molecules of N₂ are in a 500.0 mL container at 780 mm Hg and 135°C?

A 75.0 L steel tank at 20.0°C contains acetylene gas,C₂H₂,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank?

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains CH₄,flask B contains CO₂,flask C contains N₂.Which flask contains the largest number of molecules?