Chem 10-12

The heat of fusion for water is 334 joules/g, and the specific heat of water is 4.148 Jcal/g C. How many joules of heat are released when 20.0g of water at 30 C is cooled to 0.0 C and frozen to ice at 0.0 C?

-9200 J

When 35 mL of 0.92 M H2SO4 reacts with excess Al, how many L of H2 is formed at 23 C and a pressure of 745 mmHg? 2Al + 3H2SO4 --> Al2(SO4)3 + 2 H2

.80 L

What volume of H2 (at 750 mmHg and 25 C) is produced from 50.0 mL of 0.214 M H2SO4 and 0.300 g of Al? 2Al + 3H2SO4 --> Al2(SO4)3 + 2 H2

0.265 L

How many g Al will react with 24.0 mL of 1.22 M H2SO4? 2Al (s) + 3 H2SO4 (aq) → Al2(SO4)3 (aq) + 3 H2 (g)

0.527gAl

How many moles of CaCl2 are in 250 mL of a 3.00 M of CaCl2 solution

0.750 mol

A Cyclopropane-oxygen Mixture Is Used As An Anesthetic. If The Partial Pressure Of Cyclopropane In The Mixture Is 334 Mm Hg And The Partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr?

1 110

Calculate the molality of the solution formed when of 50.0 g of glucose (Molar mass 180.2) is dissolved in 0.250 kg of water.

1.11M

What is the density of carbon dioxide as STP?

1.96 g/L

What is the concentration (m/m %) of a solution of 10.0 g of sodium chloride in 100g of solution?

10.0%

The mass/mass percent concentration refers to the number of grams in a solute

100g of solution

If heat of vaporization for water is 2260 joules/g, how many kilojoules are released when 5.00 g of steam are converted to liquid at 100C?

11.3 kJ

When 25.0 g of NaCl is added to 175 g of water, the m/m % NaCl is ________.

12.5%

If the heat of fusion for water is 334 joules/g, how many kilojoules are lost when 45.0 g of water at 0.0 C is converted to ice at 0.0 C?

15.0 kJ

What is the molarity of a solution which contains 58.4g of sodium chloride dissovled in 500 mL of solution

2.00M

At STP, what is the volume of 1.0 mol of carbon dioxide?

22.4 L

At STP, temperature and pressure have the values of

273 K and 760 mmHg

At STP conditions, 11.0 g of SO2 have a volume of ____.

3.85 L

The heat of fusion for water is 334 Jg and its heat of vaporization is 2260 J/g. How many joules are required to convert 10.0 g of ice at 0.00 C to steam at 100 C? The specific heat of water is 4.184 J/g C

30 100 J

How many kilojoules are required to warm 15.0g of water from 75.0 C to 100.0 C and convert it to steam at 100.0 C? The heat of vaporization of water is 2260 J/g, and the specific heat of water is 4.184 J/g C

35.5

A container of variable volume contains oxygen gas a pressure of 550.0 kPa. at 25.0 C, what is the new pressure inside the container if the container is allowed to expand from an initial volume of 5.20 L to a final volume to 7.25 L?

394 kPa

Calculate the molarity of 60.05 g of acetic acid, HC2H3O2, dissolved in 0.250 L of solution.

4.00M

How many grams of chlorine gas are present in a 150. liter cylinder of chlorine held at a pressure of 1.00 atm and 0. °C?

474g

What is the volume of 50.0 g of N2 gas at a pressure of 650. mmHg and a temperature of 15 °C?

49.3L

A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 40.0 °C. What was the pressure in the gas tank then?

5.63 atm

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr?

528 mL

How many kilojoules are required to convert 115.0 g of ice at 0.0 C to liquid water at 32.0 C? The heat of fusion of water is 334 J/g, and the heat capacity of water is 4.184 J/g C

53.8 kJ

How many mL of 1.15 M KOH solution are needed to provide 0.665 mol of KOH?

578mL

A rigid ball that contained 25.0 liters of air at 22 °C and 6.25 atm pressure was placed in an oven at a temperature of 100. °C.What was the new pressure inside the ball?

7.90atm

A 10 liter balloon was taken from a temperature of 25 C and placed in a freezer at a temperature of -15 C. what was the new volume if pressure is constant?

8.66 liters

A molecule contains a central atom with two identical bonds to other atoms and two lone pairs. The shape of this molecule is ____.

Bent

Hydrogen bonds are a major factor in the structure of

DNA

The main interactions between molecules of methane, CH4, are ____.

Dispersion forces

ability of an atom to attract the shared electrons in a covalent bond is its

Electronegativity

Ammonia is a nonpolar molecule. True False

False

Fats are the building blocks of proteins. True False

False

For most solids, solubility decreases as the temperature of the solution increases True False

False

Sodium acetate is a weak electrolyte True False

False

Steam at 100 C holds the same amount of heat as water at 100 C True False

False

Steam at 100 °C holds the same amount of heat as water at 100 °c. True False

False

The carbon dioxide molecule contains a triple covalent bond True False

False

The m/m % concentration of a solution is the mass of the solution divided by its volume multiplied by 100

False

The m/m % concentration of a solution is the mass of the solvent divided by its volume multiplied by 100. True False

False

The pressure exerted by a gas on its container is inversely releated to its Kelvin temperature True False

False

Which of the following molecules can form hydrogen bonds

H20

Water is a polar solvent and hexane is a nonpolar solvent. Which of the following correctly describes the solubility of a the solute?

NaHCO3, soluble in water

The HF molecule can be classified as ____.

Polar covalent

In the kinetic molecular theory of gas behavior, particles of gas tend to move ___ and collision between them are ___.

Rapidly, elastic

The VSEPR theory allows us to determine the ______.

Shape of the molecule

When a solid is converted directly to a gas, the change of state is called

Sublimation

A solution with 58.5 g sodium chloride dissolved in 500.0 mL of water is 2.00 molar. True False

True

At 0 K, all motion stops True False

True

Gas law calculations normally require the use of the Kelvin temperature scale True False

True

Gas law calculations normally require the use of the Kelvin temperature scale. True False

True

Glucose is a nonelectrolyte. True False

True

Hydrochloric acid is a strong electrolyte. True False

True

If water is added to 100 mL of a 6.00 M CaCl2 solution until the volume is 200 mL, the new molarity is 3.00 M True False

True

N2 is held together by a multiple covalent bond True False

True

Sodium Acetate (NaC2H3O2) is soluble in water True False

True

The air we breathe is about 21% oxygen. True False

True

The higher the pressure of a gas above a liquid in a closed container, the greater the solubility of the gas True False

True

The kinetic energy of a gas sample is directly proportional to the Kelvin temperature of the gas True False

True

The m/m % concentration of a solution is the mass of the solute divided by the solution mass multiplied by 100 True False

True

The solubility of a gas in water decreases as the temperature increases. True False

True

When a liquid is boiling, its temperature does not change True False

True

total number of valence electrons in the fluorine molecule, F2, is 14 True False

True

What is the molarity of the solution obtained when 0.100 mol of copper sulfate are dissolved in 0.200 liters of solution? a. 0.500 M b. 0.200 M c. 0.100 M d. 0.0200 M e. 0.0500 M

a. 0.500 M

At 570. mmHg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C? a. 1560 mmHg b. 210 mmHg c. 7000 mmHg d. 690 mmHg e. 470 mmHg

a. 1560 mmHg

What is the molarity of a solution containing 5.00 moles of KCl in 2.00 L of solution? a. 2.50 M b. 1.00 M c. 5.00 M d. 10.0 M e. 2.00 M

a. 2.50 M

A 2.35 g sample of KClO3 is reacted. How many mL of O2gas is produced at a pressure of 740. mmHg and a temperature of 25 °C? 2KClO3 (s) → 2KCl (s) + 3O2(g) a. 722 mL b. 0.482 mL c. 482 mL d. 22.4 mL e. 60.7 m L

a. 722 mL

Which is the most polar bond in the following list? a. O-H b. S-O c. C-S d. I-I e. P-H

a. O-H

Which of the following correctly describes the process of inspiration (air entering the lungs)? a. The lungs expand, causing their internal pressure to decrease. b. The lungs expand, causing their internal pressure to increase. c. The lungs contract, causing their internal pressure to decrease. d. The lungs contract, causing their internal pressure to increase. e. There is no change in the internal pressure in the lungs.

a. The lungs expand, causing their internal pressure to decrease.

As you rise higher in Earth's atmosphere, the atmospheric pressure ________. a. increases b. decreases c. remains the same

a. increases

Vinegar is a solution of acetic acid (melting point 16.5 °C) in water. At room temperature(25 °C), vinegar is an example of a ________ solution. a. liquid-liquid b. gas-liquid c. solid-liquid d. solid-solid e. liquid-solid

a. liquid-liquid

The molarity (M) of a solution refers to a. moles of solute/L of solution. b. moles of solute/L of solvent. c. moles of solute/100 mL of solution. d. grams of solute/100 mL of solution. e. grams of solute/L of solution.

a. moles of solute/L of solution.

Identify as polar or nonpolar: water a. polar b. nonpolar

a. polar

The force of gas particles against the walls of a container is called ________. a. pressure b. volume c. temperature d. quantity of gas e. density

a. pressure

When two or more equivalent dot structures can be written for a given molecule it is said to have ________ structures. a. resonance b. equal c. identical d. polar e. electronegative

a. resonance

The NO3- ion is an example of a polyatomic ion with ________. a. resonance structures b. triple bonds c. a linear shape d. a nonpolar bond e. no covalent bonds

a. resonance structures

In the reaction of silver nitrate and sodium chloride to produce solid silver chloride, sodium ions and nitrate ions are ________. a. spectator ions b. solvents c. molecules d. gases e. liquid

a. spectator ions

During the process of diluting a solution to a lower concentration, a. the amount of solute does not change. b. the amount of solvent does not change. c. there is more solute in the concentrated solution. d. the volume of the solution does not change. e. water is removed from the concentrated solution.

a. the amount of solute does not change.

The pressure exerted by the particles of vapor above a liquid is called the ________ pressure. a. vapor b. barometric c. standard d. molar e. atmospheric

a. vapor

A barometer is a device for measuring ___.

atmospheric pressure

The volume of a gas with a pressure of 1.2 atm increases from 1.0 L to 4.0 L. What is the final pressure of the gas, assuming constant temperature? a. 1.2 atm b. 0.30 atm c. 3.3 atm d. 4.8 atm e. 1.0 atm

b. 0.30 atm

If the heat of fusion for water is 334 joules/g, how many kilojoules are needed to melt 45.0 g of ice at 0 °C? a. 0.0 kJ because no temperature change takes place. b. 15.0 kJ c. 15 000 kJ d. 150 kJ e. Undetermined - you need to know the final temperature.

b. 15.0 kJ

How many covalent bonds will an oxygen atom normally make? a. 1 b. 2 c. 3 d. 4 e. 5

b. 2

What is the molarity of a solution that contains 2.35 g of NH3 in 0.0500 L of solution? a. 27.6 M b. 2.76 M c. 47.0 M d. 0.276 M e. 1.00 M

b. 2.76 M

A 5.00 g sample of Al reacts with excess H2SO4. What volume of H2 gas is produced at STP? 2Al(s) + 3 H2SO4 (aq)→ Al2(SO4)3 (aq) + 3 H2 (g) a. 0.278 L b. 6.23 L c. 4.14 L d. 22.4 L e. 67.2 L

b. 6.23 L

Which of the following compounds contains a polar covalent bond? a. NaF b. HCl c. Br2 d. MgO e. O2

b. HCl

According to Henry's law, the solubility of a gas in a liquid a. decreases as the gas pressure above the liquid increases. b. increases as the gas pressure above the liquid increases. c. remains the same as the temperature increases. d. depends on the liquid polarity. e. depends on the liquid density.

b. increases as the gas pressure above the liquid increases.

Ammonium chloride, NH4Cl, is ________ in water. a. insoluble b. soluble c. a non electrolyte d. a solid e. a gas

b. soluble

In Gay-Lussac's law, the pressure of a gas increases due to an increase in temperature because a. the molecules strike the walls of the container less often. b. the molecules strike the walls of the container harder and more often. c. the molecules get bigger. d. there is a decrease in the volume of the container. e. there is an increase in the number of gas particles.

b. the molecules strike the walls of the container harder and more often.

According to the kinetic molecular theory of gases, a gas can be compressed much more than a liquid or solid because a. a gas is composed of very small particles. b. the particles of a gas are very far apart. c. gas particles move rapidly. d. gas particles do not attract or repel one another. e. gas particles move faster when the temperature increases.

b. the particles of a gas are very far apart.

What is the concentration, in m/m %, of a solution prepared from 500. g NaCl and 2.50 kg of water? a. 0.167% b. 1.67% c. 16.7% d. 0.050% e. 20.0%

c. 16.7%

How many joules are required to convert 16.5 g of ice at 0.0 °C to liquid water at 32.0 °C? The heat of fusion of water is 334 J/g. a. 5 510 J b. 2 210 J c. 7 720 J d. 1 320 J e. 334 j

c. 7 720 J

The building blocks of proteins are a. fatty acids. b. carbohydrates. c. amino acids. d. steroids. e. not known.

c. amino acids

The shape of a molecule of water, H2O, is ________. a. linear b. tetrahedral c. bent d. pyramidal e. trigonal planar

c. bent

A solution containing a large concentration of dissolved ions can be classified as a(n) ________. a. weak solution b. suspension c. electrolyte d. unsaturated solution e. solvent

c. electrolyte

The main interactions between molecules of ammonia, NH3, are ________. a. ionic bonds b. dispersion forces c. hydrogen bonds d. dipole-dipole attractions e. none of the above

c. hydrogen bonds

A burn from steam at 100 °C is expected to be more severe than a burn from boiling water at 100°C because a. the steam is hotter than the boiling water. b. there is more steam than water. c. the steam will give off a large amount of heat as it condenses. d. you are more likely to come into contact with the steam than with the boiling water. e. All of these answers are correct.

c. the steam will give off a large amount of heat as it condenses.

A molecule has a central atom and three identical bonds to other atoms, with no lone pairs. The shape of this molecule is ________. a. linear b. bent c. trigonal planar d. trigonal pyramidal e. tetrahedral

c. trigonal planar

When KCl dissolves in water

d) the K+ ions are attracted to the partially negative Oxygen atoms of the water molecule

How many moles of neon occupy a volume of 14.3 L at STP? a. 36.7 moles b. 32.0 moles c. 6.45 moles d. 0.638 moles e. 1.57 moles

d. 0.638 moles

A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg? a. 1.50 mmHg b. 507 mmHg c. 760 mmHg d. 1 140 mmHg e. 7.50 mmHg

d. 1 140 mmHg

The solubility of KI is 50. g in 100. g of H2O at 20 °C. If 110. grams of KI are added to 200. grams of H2O, a. all of the KI will dissolve. b. the solution will freeze. c. the solution will start boiling. d. a saturated solution will form. e. the solution will be unsaturated.

d. a saturated solution will form.

When the weak electrolyte HF is dissolved in water, the solution contains ________. a. all HF molecules b. all H+ and F- ions and no HF molecules c. nothing d. mostly HF molecules and a few H+ and F-ions e. only F- ions

d. mostly HF molecules and a few H+ and F-ions

A heating curve illustrates a. what a substance looks like as it is heated. b. what happens to the particles of a substance as it is heated. c. what happens to the heat applied as the temperature is increased. d. the changes in the temperature and physical state of a substance as it is heated. e. the chemical changes that occur as the substance is heated.

d. the changes in the temperature and physical state of a substance as it is heated.

The diatomic molecule N2 is held together by a ________ covalent bond. a. double b. single c. ionized d. triple e. polar

d. triple

At 26 °C, the solubility of sodium chloride is 36 g/100 mL of solution. How would you describe a solution of 10 g of sodium chloride in 100 mL of solution at room temperature? a. saturated b. a nonelectrolyte c. nonionic d. unsaturated e. a suspension

d. unsaturated

Complete the following statement: In Charles' law, the volume of gas ___ when the ___ decreases

decreases, temperature

Calculate the freezing point of a 2.00 molal solution of the nonelectrolyte glucose. The freezing point constant for water is 1.86 °C/molal. a. -2.00 °C b. 1.86 °C c. 3.72 °C d. -1.86 °C e. -3.72 °C

e. -3.72 °C

At constant temperature, a sample of helium at 760. torr in a closed container was compressed from 5.00 L to 3.00 L. What was the new pressure exerted by the helium on its container? a. 800. torr b. 2 280 torr c. 15.0 torr d. 3 800 torr e. 1 270 torr

e. 1 270 torr

How many moles of oxygen are present in a cylinder of 25.0 liters at a temperature of 0. °C and a pressure of 1.00 atm? a. 0.781 mol b. 25.0 mol c. 10.9 mol d. 0.896 mol e. 1.12 mol

e. 1.12 mol

The pressure of 5.00 L of gas increases from 1.50 atm to 1240 mmHg. What is the final volume of the gas, assuming constant temperature? a. 4120 L b. 5.00 L c. 0.00600 L d. 5.40 L e. 4.60 L

e. 4.60 L

What mass of a 15.0% (m/m) NaOH solution contains 125 g NaOH? a. 18.0 g b. 0.120 g c. 12.0 g d. 120. g e. 833 g

e. 833 g

Of the five elements Na, Al, S, Cl, F, the most electronegative is ________. a. Na b. Al c. S d. Cl e. F

e. F

Proteins are a. chains of amino acids. b. important biological molecules. c. transport molecules in the body. d. part of the structural components in the body. e. all of the above

e. all of the above

The three dimensional shape of a protein a. is important to its function. b. is determined by the attractive forces. c. can be lost when the protein is heated. d. can be lost when acid is added to the protein. e. all of the above

e. all of the above

The total pressure in a mixture of gases is equal to the partial pressure(s) of a. the gas with the greatest number of moles. b. the gas with the smallest number of moles. c. the gas with the highest molecular weight. d. the gas that occupies the largest volume. e. all the gases added together.

e. all the gases added together.

According to Avogadro's law, the volume of a gas a. is inversely related to the number of moles at constant temperature and pressure. b. is inversely related to the number of moles at standard temperature and pressure. c. depends only on the temperature and pressure. d. depends only on the number of moles in the sample. e. is directly related to the number of moles at constant temperature and pressure.

e. is directly related to the number of moles at constant temperature and pressure.

An increase in the temperature of a solution usually

increases the solubility of a solid solute in the solution

An autoclave is used to sterilize surgical equipment because

it allows water to boil at temperatures above 100 C

Identify as polar or nonpolar: carbon dioxide

nonpolar

The bond in Cl2 is a(n)

nonpolar covalent bond

Oil does not dissolve in water because

oil is nonpolar

A solid that comes out of a solution as its solubility is exceeded is called a

precipitate

Ozone, O3, is an example of a molecule that has ________ structures.

resonance

Acetic acid can be classified as a ________.

weak electrolyte