Deck 10: Chemistry of Explosions

Question 1

Calculate the volume of 3.97 mol of methane gas at STP.

A) 0.177 L
B) 5.56 L
C) 5.64 L
D) 88.9 L

Answer 1

88.9 L

Question 2

Calculate the missing variable in the following experiment using Gay-Lussac's law. P₁ = 1.57 atm, T₁ = 287 K, P₂ = ?, T₂ = 305 K

A) 0.0000180 atm
B) 1.67 atm
C) 2.20 atm
D) 137000 atm

Answer 2

1.67 atm

Question 3

Determine how many moles of oxygen would be necessary for the complete oxidation of two moles of C₄H₁₀ to CO₂ and H₂O.

A) 3
B) 9
C) 13
D) 17

Answer 3

13

Question 4

What happens to the volume of a gas when the amount of the gas doubles and all other variables are constant?

A) The volume increases.
B) The volume decreases.
C) The volume stays the same.

Question 5

Calculate the missing variable in the following experiment using Charles's law. V₁ = 6.35 L, T₁ = 342 K, V₂ = ?, T₂ = 278 K

A) 0.0000668 L
B) 5.16 L
C) 7.81 L
D) 604000 L

Question 6

Calculate the missing variable in the following experiment using Avogadro's law: V₁ = 1.50 L, n₁ = 3.95 mol, V₂ = ? L, n₂ = 0.891 mol

A) 0.338 mol
B) 0.426 mol
C) 2.96 mol
D) 6.64 mol

Question 7

Calculate the missing variable in the following experiment using Gay-Lussac's law. P₁ = 3.88 atm, T₁ = 278 K, P₂ = 2.98 atm, T₂ = ?

A) 0.0416 K
B) 213 K
C) 362 K
D) 3210 K

Question 8

Determine whether TNT (C₇H₅N₃O₆) has a negative, neutral, or positive oxygen balance.

A) negative
B) neutral
C) positive

Question 9

Calculate the volume of 49.2 g of carbon dioxide at STP.

A) 1.12 L
B) 20.0 L
C) 25.0 L
D) 1100 L

Question 10

A gas initially occupies 4.50 L at 23°C and 1.50 atm. Calculate its volume after the temperature is increased to 160°C and the pressure is decreased to 0.50 atm.

A) 0.0000263 L
B) 0.0506 L
C) 9.23 L
D) 19.7 L

Question 11

Calculate the missing variable in the following experiment using Boyle's law: V₁ = 0.890 L, P₁ = 2.19 atm, V₂ = ?, P₂ = 0.376 atm

A) 0.193 L
B) 0.733 L
C) 1.08 L
D) 5.18 L

Question 12

Calculate the missing variable in the following experiment using Charles's law. V₁ = 10.25 L, T₁ = 300 K, V₂ = 4.98 L, T₂ = ?

A) 0.00162 K
B) 0.170 K
C) 146 K
D) 617 K

Question 13

What happens to the pressure of a gas when the temperature of the gas decreases and all other variables are constant?

A) The pressure increases.
B) The pressure decreases.
C) The pressure stays the same.
Enter the appropriate word(s) to complete the statement.

Question 14

What is the pressure of a 15.0-L compressed gas tank that holds 17.8 mol of carbon dioxide gas at 375 K?

A) 0.0274 atm
B) 0.0584 atm
C) 36.5 atm
D) 3850 atm

Question 15

Which of the following statements is not a part of the kinetic molecular theory of gases?

A) Gas particles are extremely small and have relatively large distances between them.
B) The average kinetic energy of gas particles is proportional to the pressure of the gas.
C) Gas particles are in continuous random, straight-line motion as they collide with one another and with the container walls.
D) Gas particles act independently of one another because there are no significant attractive or repulsive forces between gas particles.

Question 16

Which statement gives a difference between a low explosive and a high explosive compound?

A) Only a high explosive compound contains nitrogen.
B) A high explosive compound will explode without being confined.
C) A low explosive is less dangerous than a high explosive compound.
D) A high explosive compound must be ignited at a higher temperature than a low explosive.

Question 17

A mixture of oxygen, hydrogen and nitrogen gases exerts a total pressure of 2.74 atm. If the partial pressures of the oxygen and the hydrogen are 1.11 atm and 0.997 atm respectively, what would be the partial pressure exerted by the nitrogen?

A) 0.633 atm
B) 2.63 atm
C) 2.85 atm
D) 4.85 atm

Question 18

A gas-tight syringe is filled to 20.0 mL, at a pressure of 1.15 atm and 24.0°C, with one of the noble gases. If the mass of the empty syringe is 58.902 g and the mass of the filled syringe is 59.026 g, identify the noble gas contained in the syringe.

A) Ar
B) Kr
C) Xe
D) Rn

Question 19

Calculate the missing variable in the following experiment using Boyle's law: V₁ = 2.50 L, P₁ = 0.590 atm, V₂ = 3.40 L, P₂ = ?

A) 0.434 L
B) 1.25 L
C) 2.31 L
D) 5.02 L

Question 20

Calculate the missing variable in the following experiment using Avogadro's law: V₁ = 4.20 L, n₁ = 0.753 mol, V₂ = 2.93 L, n₂ = ?

A) 0.525 mol
B) 1.90 mol
C) 9.27 mol
D) 16.3 mol

Question 21

Calculate the density of 1 mol of hexane at STP.

Question 22

Calculate the total pressure of an 8.00-L container at 23°C that contains 75 g of xenon and 55 g of nitrogen gas.