Chem Final pt4

For a constant quantity of gas at constant pressure, when temperature decreases, volume _____.

decreases

For a constant quantity of gas at constant temperature, when volume decreases, pressure _____.

increases

For a given quantity of gas in a container with a fixed volume, when temperature increases, pressure _____.

increases

Which gas law focuses on the relationship between pressure and volume?

Boyle’s Law

Which of the following represents standard temperature and pressure?

0°C and 101.325 kPa

What volume does any gas occupy at STP?

22\.4L

A gas that behaves according to the kinetic-molecular theory is a(n) _____ gas.

ideal

In the equation PV = nRT, n represents the number of ____ in a sample.

moles of gas

Which gas law is represented by the equation PV = nRT?

the ideal gas law

What volume will 2.50 mol of a gas occupy at 283 K and a pressure of 40.0 kPa?

147L (pg 2

How many moles of a gas are present in a 5.2 L sample at 202.68 kPa of pressure and 278.15 K?

What is the volume of 2.50 mol of nitrogen at STP?

56\.0L

The intermolecular forces that exist between polar molecules only are _____.

dipole-dipole forces

Hydrogen bonds can occur between molecules containing hydrogen and _____.

oxygen

The fact that water is a liquid at room temperature is best explained by the existence of _____.

hydrogen bonds

The compound NH3 demonstrates which of the following kinds of intermolecular forces?

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a) hydrogen bonds

b) London dispersion forces

c) both a and b

d) neither a nor be

c

Which of the following occurs when particles vibrate vigorously during heating, causing attractive forces to be overcome?

sublimation

What occurs when individual molecules leave the surface of a solid and become gaseous?

sublimation

What is the process in which gas molecules collect to form a solid?

deposition

Which of the following is not one of the seven basic classes of crystals?

a) triclinic

b) hexagonal

c) quadrilateral

d) rhombohedral

c) quadrilateral

What is released when gaseous particles form crystals?

lattice energy

Which of the following statements is not true of solutions?

a) They are uniform.

b) They can vary in concentration.

c) Their solutes will settle out after long periods.

d) They are mixtures.

c) Their solutes will settle out after long periods.

A solution is a _____.

homogeneous mixture

In a solution of two substances, the component present in the larger amount is known as the _____.

solvent

In a solution of two substances, the component present in the smaller amount is known as the _____.

solute

If one liquid is soluble in another and can form a solution, the two liquids are said to be _____.

miscible

What type of solution can gold and mercury form?

solid-liquid

What is the solvent in the air that we breathe?

nitrogen

Which of the following statements is true?

a) The first steps of solvation release thermal energy, whereas the mixing process absorbs it.

b) All aspects of solvation release thermal energy.

c) The first steps of solvation absorb thermal energy, whereas the mixing process releases it.

d) All aspects of solvation absorb thermal energy.

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c) The first steps of solvation absorb thermal energy, whereas the mixing process releases it.

When water is the solvent, the process of solvation is called _____.

hydration

The net energy change during the solution process is measured as the _____ of solution.

enthalpy

Crystalline substances with high lattice energies that dissociation cannot overcome are _____.

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insoluble

What is the general rule that governs whether substances will form solutions together?

Like dissolves like.

Which of the following is insoluble in water?

a) KF

b) KNO3

c) NaBr

d) CH4

d) CH4

A solution that contains the maximum amount of solute at a given temperature is _____.

saturated

If the solubility of NaCl in water is 35.9 g/100 mL (at 25 °C), how would you describe a 100 mL solution that contains only 30.0 g NaCl?

unsaturated

How many moles of sodium hydroxide (NaOH) need to be dissolved in 2.00 L of water to produce a 0.50 M NaOH solution?

1\.00 mol (pg. 340)

What is the amount concentration of a solution that contains 0.85 mol of solute in 352 mL of solution?

2\.41 mol/L (pg. 340)

The average kinetic energy in the particles of a sample is that substance's _____.

temperature

Which branch of science studies the transfer of energy during chemical reactions or phase changes?

thermochemistry

Enthalpy is a measure of _____ at a constant pressure.

thermal energy

On a heating curve, the thermal energy represented by the horizontal portion of the curve is _____ heat.

latent

The heat that produces a phase change is called _____ heat.

latent

The amount of heat required to convert 1 mol of liquid at its boiling point to its vapor at the same temperature is called its molar enthalpy of _____.

vaporization

Ammonia has a molar enthalpy of vaporization of 23.3 J/mol. Water's enthalpy of vaporization is 40.7 kJ/mol. What can we deduce from these figures?

There are stronger intermolecular attractions between water molecules than between ammonia molecules (pg. 359).

How much heat is required to melt 200.0 g of ice given that the heat of fusion of ice is 6.01 kJ/mol?

66\.7 kJ (pg. 359)

What symbol represents specific heat?

specific heat

Csp

The specific heat of copper is 0.39 J/(g • °C), and that of silver is 0.23 J/(g • °C). Which metal would have the higher temperature if the same amount of thermal energy were added to 50.0 g of each metal?

silver

A sour taste is associated with _____.

Acids

Any substance that ionizes to conduct electricity in a solution is called a(n) _____.

electrolyte

If a substance turns red litmus paper blue, it is a(n) _____.

base

A base usually feels _____.

slippery

Most bases taste _____.

bitter

Which of the following hydrogen-containing compounds is not an acid?

a) HC2H3O2

b) HCHO2

c) HS

d) CH4

d) CH4