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Flashcards in Ch. VI Deck (31):
1

Molecules are farthest apart in a(n)

gas

2

Liquids are

difficult to compress and have no definite shape

3

When a liquid changes into a gas, the process is called

vaporization

4

When a liquid changes into a solid, the process is called

freezing

5

When a solid changes directly into a gas, the process is called

sublimation

6

Which of the following is not composed of particles that exhibit intermolecular forces?

NaBr

7

Which of the following solids is likely to require the greatest input of energy to melt?

KBr

8

What intermolecular forces are most significant in accounting for the high boiling point of liquid water relative to other substances of similar molecular weight?

Hydrogen bonds

9

Which of the following interactions is the strongest?

Covalent bonds

10

In ethanol (CH3CH2OH), the attractions between neighboring molecules are

hydrogen bonds, dipole-dipole forces, and dispersion forces only

11

The molecules of liquid water in a beaker are held to each other by

intermolecular forces

12

Of CH3OH, H2, HF, and H2O, which molecule(s) can form hydrogen bonds?

CH3OH, HF, and H2O

13

Which one of the following molecules does NOT form hydrogen bonds?

Chloroform (CHCl3)

14

A solution is a mixture that is

homogeneous

15

Which of the following pairs of substances is least likely to form a solution?

An ionic compound in a nonpolar solvent

16

A positive test for iodine is the purple color of a solution of I2 in hexane (C6H14). What type of solute-solvent interaction is the most important in a solution of nonpolar I2 in nonpolar C6H14?

Dispersion forces

17

What type of solute-solvent interaction is most important in a solution of calcium chloride (CaCl2) in water?

Ion-dipole interactions

18

What type of solute-solvent interaction is most important in a solution of acetic acid (CH3COOH) in water?

Hydrogen bonds

19

Which of the following solutes is most likely to dissolve in octane (C8H18), a compound of gasoline?

CH3 (CH2)4 CH3

20

Which of the following is not a concept of the kinetic-molecular theory of gases?

The pressure and volume of a gas are inversely related.

21

According to the kinetic-molecular theory of gases, a gas particle

is tiny compared to the volume occupied by the gas

22

In collisions between gas particles, the total energy

remains the same

23

Gas pressure is caused by

gas molecules colliding with vessel walls

24

Boyle's law states that the pressure of a gas is inversely proportional to its

volume

25

A gas sample occupies 6 L at 2 atm pressure. At what pressure would the volume be 1.5 L if the temperature remains constant?

8 atm

26

In an experiment, as the temperature is changed at constant pressure, the volume of a gas is halved. How is the final temperature related to the initial temperature?

The Kelvin temperature is halved.

27

One 1-L flask (Flask A) contains no gas, and another 1-L flask (Flask B) contains NO2 gas, both at STP. Flask A contains

less mass but the same number of molecules as Flask B

28

How many moles are there in 5.6 L of gas at STP?

.25 mol

29

In the ideal gas equation, PV=nRT, the variable n stands for

the number of moles

30

At STP, 1 mol of an ideal gas occupies 22.4 L. What volume does 1 mol of an ideal gas occupy at 20 °C and 1.5 atm?

16 L

31

The molar volume of an ideal gas at 2 atm and 546 K is

22.4 L