Chemistry Final

5.21 cm us the same distance as A) 0.0521 m B) 52.1 m C) 5.21 mm D) 0.00521 km E) 5210 m

A

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27 °C, if the moles are constant? A) 580 mL B) 630 mL C) 100 mL D) 110 mL E) 1100 mL

A

A dose of aspirin of 5.0 mg per kilogram of body weight has been prescribed to reduce the fever of an infant weighting 8.5 pounds. The number of milligrams of aspirin that should be administrated is A) 19 mg B) 53 mg C) 1.6 mg D) 5.0 mg E) 0.59 mg

A

A hydrogen bond is A) an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule. B) a covalent bond between H and O. C) an ionic bond between H and another atom. D) a bond that is stronger than a covalent bond. E) the polar O-H bond in water.

A

A polar covalent bond is found in which of these compounds? A) H20 B) F2 C) NaCl D) H2 E) N2

A

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, if the moles are constant? A) 530 mL B) 450 mL C) 970 mL D) 240 mL E) 400 mL

A

A solution is prepared by dissolving 2 g of NaCl in 100 g of H2O. In this solution, NaCl is the A) solute. B) solvent. C) solution. D) solid. E) ionic compound.

A

A tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm? A) 2.1 atm B) 0.55 atm C) 1.0 × 103 atm D) 1.5 atm E) 1600 atm

A

An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions. How many grams of Ca2+ are in 3.0 L of the solution? A) 0.24 g B) 0.80 g C) 0.40 g D) 240 g E) 4.0 g

A

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

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules A) move rapidly in random directions. B) are attracted to each other by strong forces. C) are close together in their container. D) move with a kinetic energy equal to their centigrade temperature. E) occasionally come to rest.

A

In water, a substance that partially ionizes in solution is called a A) weak electrolyte. B) nonelectrolyte. C) semiconductor. D) nonconductor. E) strong electrolyte.

A

The ammonia molecule (NH3) is A) polar molecule with polar bonds B) a non polar molecule with polar bonds C) a non polar molecule with non polar bonds D) a polar molecule with non polar bonds E) a polar molecule with ionic bonds

A

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

What Is the formula of a compound that contains Na+ and PO4 3- ions? A) Na3PO4 B) NaPO4 C) Na2PO3 D) Na3PO3 E) Na3P

A

What is oxidized and what is reduced in the following reaction? 2Al(s) + 3Cl2(g) ----> 2AlCl3(s) A) Al is oxidized and Br2 is reduced B) AlBr3 is reduced and Br2 is oxidized C) Al is reduced and Br2 is oxidized D) AlBr3 is reduced and Al is oxidized E) AlBr3 is oxidized and Al is reduced

A

What is the electron configuration for Aluminum? A) 1s^2 2s^2 2p^6 3s^2 3p^1 B) 1s^2 2s^2 2p^6 3s^2 3p^3 C) 1s^2 2s^2 2p^6 3s^2 3p^5 D) 1s^2 2s^2 2p^6 3s^2 3p^6 E) 1s^2 2s^2 2p^6 3s^2 3p^8

A

What is the mass of a sample of O2 gas, which has a pressure of 740.mmHg, at a temperature of 25 °C, in a volume of 250. mL? A) 0.318 g B) 3.82 g C) 201 g D) 292 g E) 320. g

A

What is the mass of a sample of O2 gas, which has a pressure of 740.mmHg, at a temperature of 25C, in a volume of 250. mL? A) 0.318 g B) 3.82 g C) 201 g D) 292 g E) 320 g

A

What is the mass of neon that exerts a pressure of 720. mmHg,with a temperature of -15.0 °C , when the volume of the container is 760. mL? A) 0.0340 g B) 0.686 g C) 0.615 g D) 517 g E) 25.8 g

A

What is the new mass/volume (m/v)% of a KOH solution that is prepared by diluting 110 mL of a 6% (m/v) KOH solution to 330 mL? A) 2% B) 1% C) 6% D) 12% E) 18%

A

Which combination of non metals exists as diatomic molecules at room temperature? A) chlorine and oxygen B) Bromine and carbon C) nitrogen and potassium D) oxygen and sodium E) fluorine and boron

A

Which of the following elements has the lowest electronegativity? A) Li B) C C) N D) O E) F

A

Which of the following polyatomic ion combination has a (1-,3-) ionic charge? A) hydroxide, phosphate B) sulfate, phosphate C) sulfate, bicarbonate D) carbonate, hydroxide E) carbonate, phosphate

A

A homogeneous mixture that does not settle out upon standing is A) an element. B) a colloid. C) a suspension. D) homogeneous. E) hydrated.

B

A slice of pizza contains 29 g of carbohydrate, 13 g of protein and unknown amount of fat. If the pizza contains 280 kcal, how many grams of fat are present? A) 10g B) 12 g C) 25 g D) 55 g E) 250 g

B

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

According to the kinetic theory of gases, particles of a gas A) are very large. B) are very far apart. C) lose their valence electrons. D) move slowly. E) decrease kinetic energy as temperature increases

B

How many electrons will chlorine gain or lose when it forms an ion?A) lose 1 B) gain 1 C) lose 7 D) gain 2 E) lose 3

B

How many equivalents are present in 5.0 g of Al3+? A) 15 Eq B) 0.56 Eq C) 0.19 Eq D) 0.37 Eq E) 3 Eq

B

How many grams of glucose (C6H12O6) are in 3.55 moles of glucose? A) 180. g B) 639 g C) 103 g D) 426 g E) 50.7 g

B

Identify the correct order of metal, metalloid, and non-metal in the following list. A) Sulfur, aluminum, sodium B) potassium, aluminum, selenium C) boron, calcium, carbon D) chlorine, calcium, silicon, E) germanium, oxygen, strontium

B

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 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

In an electron-dot structure of an element, the dots are used to present A) All of the electrons in the atom B) The valence electrons C) The electron arrangement D) Only the electrons that will participate in the bond formation E) The electrons that the element will gain when it forms a compound

B

Oil does not dissolve in water because A) oil is polar. B) oil is nonpolar. C) water is nonpolar. D) water is saturated. E) oil is hydrated.

B

The O-H bond in water is polar because A) it is an ionic bond. B) oxygen is much more electronegative than hydrogen. C) oxygen occupies more space than hydrogen. D) hydrogen is much more electronegative than oxygen. E) it is a hydrogen bond

B

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be A) lower, because temperatures are lower. B) lower, because the atmospheric pressure is lower. C) higher, because the altitude is greater. D) higher, because there are fewer water molecules in the air. E) the same, because water always boils at 100 °C.

B

The maximum number of electrons that may occupy the second energy level is A) 2 B) 8 C) 10 D) 18 E) 32

B

The scientific notation for the combination of (0.000 00034, 2705) A) 3.4 x 10^7, 2.705 x 10^3 B) 3.4 x 10^-7, 2.705 x 10^3 C) 3.4 x 10-7, 2.705 x 10^-3 D) 3.4 x 10^-7, 2.70 x 10^3 E) 3.4 x 10^-7, 2.70 x 10^-3

B

The strongest interaction between molecules of ammonia ( NH3) are? A) Ionic bonds B) Hydrogen bonds C) Polar Covalent D) Dipole-dipole E) Dispersion forces

B

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 no change in moles or temperature? A) 1.2 atm B) 0.30 atm C) 3.3 atm D) 4.8 atm E) 1.0 atm

B

What is the concentration, in m/v percent, of a solution prepared from 50. g NaCl and 2.5 L of water? A) 5.0% B) 2.0% C) 0.020% D) 0.050% E) 20.%

B

What is the correct formula for Sodium sulfide? A) Na2S2 B) Na2S C) NaS D) NaS2 E) Na2S3

B

What is the element with the abbreviated electron configuration [Kr]5s24d8? A) Ni B) Pd C) Pt D) Kr E) Xe

B

What is the ionic charge of an ion with 12 protons and 10 electrons?A) 1+ B) 2+ C) 3+ D) 2- E)3-

B

What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL? A) 0.267 M B) 0.150 M C) 0.200 M D) 6.67 M E) 0.100 M

B

What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution? A) 34 M B) 2.0 M C) 0.50 M D) 0.029 M E) 1.0 M

B

What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution? A) 0.0400 mL B) 25.0 mL C) 2.00 mL D) 1.00 × 104 mL E) 5.00 × 102 mL

B

When 200. mL of water are added to 100. mL of 12% KCl solution the final concentration of KCl is (Assume the volumes add.) A) 12%. B) 4.0%. C) 36%. D) 6.0%. E) 8.0%.

B

When 3.05 moles of CH4 are mixed with 5.03 moles of O2 the limiting reactant isCH4 + 2O2 → CO2 + 2H2O A) CH4. B) O2. C) CO2. D) H2O.

B

Which of the following correctly gives the best coefficients for the reaction below? N2H4 + H2O2 ------> N2 + H2O A) 1,1,1,1 B) 1,2,1,4 C) 2,4,2,8 D) 1,4,1,4 E) 2,4,2,4

B

Which of the following is an example of potential energy? A) chewing gum B) water stored in a reservoir C) burning wood D) a fan blade turning E) riding an exercise bike

B

Which one of the following is NOT correct statement explaining a hypothesis? A) If I add air to a flat bicycle tire, it will expand to the proper size. B) When I add air to the bicycle tire, it was still flat. C) The bicycle tire is flat because it must have a leak in it. D) If I chop a big lod into smaller pieces, it will burn better. E) When Jim experienced a stomach cramp after drinking milk, he thinks he may be lactose intolerant

B

what is the abbreviated electron configuration for selenium (atomic number 34) A) [He] 2s2 2p3 B) [Ar] 4s23d104p4 C) [Ar] 4s23d84p3 D) [Ar] 4s13d104p4 E) [Ar] 3d8

B

36x0.12345 What is the correct answer for the calculation -------------- ? 6.77 A) 0.65645 B) 0.656 C) 0.66 D) 1.52 E) 1.5

C

A 50.0 mL urine sample has a mass of 50.7 g. The specific gravity of the urine is (SG has no units and most appropriate answer is after considering the SF) A) 1.014 g/mL B) 0.986 g/l C) 1.01 D) 0.986 E) 50.7

C

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? A) 0.625 atm B) 4.44 atm C) 5.63 atm D) 40.0 atm E) 69.5 atm

C

A group of covalently bonded atoms that has an overall electrical charge is called a(n) A) ionic compound. B) anion C) polyatomic ion. D) cation. E) molecule.

C

An increase in the temperature of a solution usually A) increases the boiling point. B) increases the solubility of a gas in the solution. C) increases the solubility of a solid solute in the solution. D) decreases the solubility of a solid solute in the solution. E) decreases the solubility of a liquid solute in the solution.

C

At STP, temperature and pressure have the values of A) 0 K and 1 atm. B) 273 K and 1 mmHg. C) 273 K and 760 mmHg. D) 0 K and 760 mmHg. E) 760 K and 273 atm.

C

How many calories are required to increase the temperature of 13 g of alcohol from 11 c to 23 c? The specific heat of alcohol is 0.588 cal/g c? A) 83 cal B) 0.63 cal C) 92 cal D) 0.54 cal E) 170 cal

C

How many grams of PbCl2 are formed when 25.0 mL of 0.654 M KCl react with Pb(NO3)2?2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s) A) 22.7 g B) 1.64 g C) 2.27 g D) 4.54 g E) 9.08 g

C

How many valence electrons are in the electron-dot structures for the elements in group 3A(13)? A) 1 B) 2 C) 3 D) 4 E) 6

C

IN which of the following would the particles move most rapidly? A) ice at -20 c B) water at 20 c C) steam at 110 c D) boiling water E) ice at 0 c

C

In a solution, the solvent A) is a liquid. B) can be a liquid or gas. C) can be a solid, liquid, or gas. D) is never a solid. E) is the substance present in the smallest concentration

C

In the kinetic molecular theory of gas behavior, particles of a gas tend to move ________ and collisions between them are ________. A) rapidly; rare B) slowly; rare C) rapidly; elastic D) slowly; elastic E) slowly; unusual

C

Of the elements: B,C,F,Li, and Na. The element with the least metallic character is? A) B B) C C) F D) Li E) Na

C

The ion of aluminum is A) Al+. B) Al2+. C) Al3+. D) Al3-. E) Al2-.

C

The number of valance electrons found in an atom of a Group A element is equal to A) its atoms number B) its mass number C) its group number D) eight E) wight minus the group number

C

The volume of a gas with an initial pressure of 380 mmHg atm increases from 5.0 L to 8.0 L. What is the final pressure of the gas,in atm, assuming no change in moles or temperature? A) 238 atm B) 2.4 atm C) 0.31 atm D) 0.80 atm E) 8.0 atm

C

Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute? A) mineral oil, soluble in water B) CaCl2, soluble in hexane C) NaHCO3, soluble in water D) CCl4, soluble in water E) octane, soluble in water

C

What is the coefficient of hydrogen, H2, when the following equation is balanced?Al + H2SO4 ------> Al2(SO4)3 + H2 A) 1 B) 2 C) 3 D) 4 E) 5

C

What is the ionic charge of an ion with 13 protons and 10 electrons?A) 1+ B) 2+ C) 3+ D) 2- E) 3-

C

What is the volume of a cube that measures 4.00 cm on each side ? A) 16.0 mL B) 64.0 L C) 64.0 Cc D) 64.00 mL E) 0.640 L

C

What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH? A) 0.075 L B) 0.25 L C) 0.75 L D) 0.083 L E) 750 L

C

When the combined gas law is rearranged to solve for P2, the following is the correct expression: P2 = A) T2T1V1/V2P1. B) P1V2T2/V2T1. C) P1V1T2/V2T1. D) V2T2/P1V1T1. E) P1V1/T1 - V2/T2.

C

Which of the following compounds contains an ionic bond? A) NH3 B) H2O C) CaO D) H2 E) CH4

C

Which of the following compounds contains an ionic bond? A) NH3 B) H2O C) K2O D) H2 E) CH4

C

Which of the following measured contains the designated CORRECT number of significant figures? A) 0.04300. 5 significant figures B) 0.00302. 2 significant figures C) 156 000. 3 significant figures D) 1.04. 2 significant figures E) 3.0650 4 significant figures

C

Which one of the following compounds contains an ion with a 3+ charge? A) KCl B) Na2O C) FeCl3 D) CuCl E) MgCl2

C

Which one of the following compounds will NOT be soluble in water? A) LiOH B) K2S C) BaSO4 D) NaNO3 E) MgCl2

C

Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) When 25.0 g of Zn reacts, how many L of H2 gas are formed at 25 °C and a pressure of 854 mmHg? A) 8.56 L B) 0.120 L C) 8.32 L D) 22.4 L E) 0.382 L

C

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) 1140 mmHg E) 7.5 mmHg

D

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K, at constant moles and volume? A) 1.5 atm B) 0.94 atm C) 0.47 atm D) 2.1 atm E) 1.1 atm

D

According to Boyle's Law, the pressure of a gas increases as the volume decreases because A) the gas particles get bigger. B) the kinetic energy of the gas particles increases. C) the temperature of the gas increases. D) the gas particles strike the walls of the container with more force. E) the gas particles strike the walls of the container more often.

D

At STP, what is the volume of 4.50 moles of nitrogen gas? A) 167 L B) 3420 L C) 101 L D) 60.7 L E) 1230 L

D

Complete the following statement: In Charles's Law, the volume of a gas ________ when the ________ decreases. A) increases; temperature B) increases; quantity of gas C) increases; pressure D) decreases; temperature E) decreases; pressure

D

How many equivalents are present in 0.40 moles of SO42-? A) 0.10 Eq B) 0.20 Eq C) 0.40 Eq D) 0.80 Eq E) 1.2 Eq

D

How many grams of H2O are needed to produce 150 g of Mg(OH)2?A) 46 g B) 18 g C) 130 g D) 93 g E) 23 g

D

How many moles of K2SO4 are in 15.0 g of K2SO4? A) 0.172 moles B) 2.61 × 103 moles C) 0.111 moles D) 0.0861 moles E) 0.119 moles

D

How many valance electrons are in the electron-dot structure of H2O A) 2 B) 4 C) 6 D) 8 E) 10

D

How many valence electrons are in the electron-dot-structure of CH4? A)2 B)4 C)6 D)8 E)10

D

Hydrogen sulfide H2S, has a shape similar to? A) Carbon dioxide B) Carbon monoxide C) Hydrogen chloride D) Water E) Carbon tetrachloride

D

Identifying correct order of names of the following elements AL, Ca, Si, S, B, Ba A) Aluminium, Carbon, srontium, sulfur, barium, boron B) Aluminum, calcium, sillicon, sulfur, barium, berryllium C) aluminium, carbon, strontium, sillicon, beryllium, barium D) aluminum, calcium, silicon, sulfur, boron, barium E) aluminium, carbon, sillicon, sulfur, boron, barium

D

In a molecule with covalent bonding A) oppositely charged ions are together by strong electrical attractions B) atoms of metals form bonds to atoms of nonmetals C) atoms are different metals form bonds D) atoms are held together by sharing electrons E) atoms are noble gasses are held together by attractions between oppositely charged ions

D

One mole of particles of any substance contains how many particles? A) 106 B) 3 × 10-10 C) 3 × 1010 D) 6.02 × 1023 E) 6.02 × 10-23

D

The compound KBr2 is named A) Potassium bromine B) Potassium dibromide C) Potassium (I) bromide D) Potassium bromide E) Monopotassium dobromide

D

The mathematical expression of the ideal gas law is A) P1V1 = P2V2. B) = C) = D) PV = nRT. E) PT = P1 + P2 + P3.

D

The name of Al(OH)3 is A) aluminum trihydroxide. B) monoaluminum trihydroxide. C) aluminum hydroxide. D) aluminum(III) hydroxide. E) aluminum oxygen hydride.

D

The number of neutrons in an atom is equal to A) the atomic number B) the mass number C) the mass number + the atomic number. D) the mass number - the atomic number. E) the number of protons

D

The octet rule indicates that A) all of the noble gases have eight total electrons B) All of the shells in an atom hold a maximum of 8 electrons C) All of the Group A elements have 8 valence electrons D) Atoms lose, gain, or share valance electrons to have 8 valance electrons E) The noble gases react with other compounds to get 8 valance electrons

D

The pressure exerted by a gas on its container is directly proportional to A) the volume of the container. B) the mass of the individual gas molecules. C) the centigrade temperature of the gas. D) the number of moles of gas in the sample. E) the Fahrenheit temperature of the gas.

D

The shape of the water molecule (H2O) is A) linear B) tetrahedral C) pyramidal D) bent E) octagonal

D

The smallest particle of an element that retains the characteristic of the element is an A) electron B) neutron C) proton D) atom E) nucleus

D

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

To form an ion, a sodium atom A) gains one electron. B) gains two electrons. C) loses seven electrons. D) loses one electron. E) loses two electrons.

D

Vapor pressure can be described as A) the temperature at which bubbles of vapor appear in a liquid. B) the pressure exerted on the Earth by the particles in the air. C) the temperature at which the vapor pressure of a liquid equals atmospheric pressure. D) the pressure exerted by a gas above the surface of its liquid. E) the pressure within the lungs during inhalation.

D

What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water? A) 0.250% B) 33.3% C) 40.0% D) 25.0% E) 3.00%

D

What is the molarity of a solution that contains 3.25 moles of NaNO3 in 250. mL of solution? A) 3.25 M B) 6.50 M C) 0.0130 M D) 13.0 M E) 2.60 M

D

When KCl dissolves in water A) the Cl- ions are attracted to dissolved K+ ions. B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule. C) the K+ ions are attracted to Cl- ions on the KCl crystal. D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule. E) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.

D

Which fo the following properties describes a liquid A) has its own shape B) particles are close together and move randomly C) particles move very rapidly D) fills the entire volume of a container E) There is essentially no interaction between the particles

D

Which of the following SI unit combination is used to measure volume and temperature? A) Cubic meter, Celcius B) Cubic centimeter, kelvin C) Liter, Kelvin D) Cubic meter, Kelvin E) Liter, Celcius

D

Which of the following gives the balanced equation for this reaction?K3PO4 + Ca(NO3)2 ------> Ca3(PO4)2 + KNO3 A) KPO4 + CaNO3 + KNO3 B) K3PO4 + Ca(NO3)2 -----> Ca3(PO4)2 + 3KNO3 C) 2K3PO4 + Ca(NO3)2 -----> Ca3(PO4)2 + 6KNO3 D) 2K3PO4 + 3Ca(NO3)2 -----> Ca3(PO4)2 + 6KNO3 E) K3PO4 + Ca(NO3)2 -----> Ca3(PO4)2 + KNO3

D

Which of the following properties is Not a characteristic of the Group 1A (1) elements (alkali metals) A) They are shiny B) they are good conductors of heat C) they react vigorously with water D) Most of them are liquids at room temperature E) they're good conductors of electricity

D

which of the following is a chemical change A) cutting rope B) bending a steel rod C) making a snowman D) burning sugar E) melting gold

D

A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 330 mmHg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the mixture in torr? A) 330 torr B) 430 torr C) 760 torr D) 1.4 torr E) 1100 torr

E

According to Avogadro's law A) the volume of a gas is inversely related to the number of moles at constant temperature and pressure. B) the volume of a gas is inversely related to the number of moles at standard temperature and pressure. C) the volume of a gas depends only on the temperature and pressure. D) the volume of a gas depends only on the number of moles in the sample. E) the volume of a gas is directly related to the number of moles at constant temperature and pressure

E

An ionic compound A) has a net positive charge. B) has a net negative charge. C) contains only cations. D) contains only anions. E) has a net charge of zero

E

At STP, how many moles of helium gas would occupy 1.00 L? A) 2.24 moles B) 224 moles C) 22.4 moles D) 0.446 moles E) 0.0446 moles

E

At constant temperature, a sample of helium at 760. torr in a closed container was compressed from 5.00 L to 3.00 L, with no change in moles or temperature. What was the new pressure exerted by the helium on its container? A) 800. torr B) 2280 torr C) 15.0 torr D) 3800 torr E) 1270 torr

E

How many mL of 0.246 M Pb(NO3)2 are needed to react with 36.0 mL of 0.322 M KCl ? 2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s) A) 36.0 mL B) 18.0 mL C) 72.0 mL D) 47.1 mL E) 23.6 mL

E

How many valence electrons does nitrogen have? A) one B) two C) three D) four E) five

E

In a __________ reaction, two or more elements or compounds form one product? A) Decomposition B) Single replacement C) Dehydration D) Double replacement E) Combination

E

In a gas, the distance between the particles is A) very close relative to the size of the molecules. B) close relative to the size of the molecules. C) fixed relative to the size of the molecules. D) small relative to the size of the molecules. E) very large relative to the size of the molecules.

E

In ionic compounds, ________ lose their valence electrons to form positively charged ________. (5,2) A) metals; anions B) nonmetals; cations C) metals; polyatomic ions D) nonmetals; anions E) metals; cations

E

Isotopes are atoms of the same element that have A) diffrent atomic numbers B) the same atomic numbers but different numbers of protons C) the same atomic numbers but different numbers of electrons D) the same atomic number but different numbers of neutrons E) the same atomic mass but different number of protons

E

Of the elements: B,C,F, Li, and Na., the element with the largest atomic radius is A) B B) C C) F D) Li E) Na

E

The correct formula for a compound formed from the elements Al and O is A) AlO. B) Al2O. C) Al3O2. D) AlO3. E) Al2O3.

E

The strongest interactions between atoms of helium He are examples of A) Ionic bonds B) Covalent bonds C) Hydrogen bonds D) Dipole-dipole interactions E) Dispersion forces

E

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

The unit of 1 atmosphere used to describe the pressure of a gas is equal to A) 1 mmHg . B) 100 mmHg. C) 200 mmHg. D) 600 mmHg. E) 760 mmHg.

E

The volume of a sample of gas, initially at 25 °C and 158 mL, increases to 450. mL. What is the final temperature of the sample of gas, if the pressure in the container is kept constant? A) 8.8 °C B) 71 °C C) 105 °C D) -168 °C E) 576 °C

E

To form an ion, a magnesium atom A) Gains one electron B) Gains two electrons C) Loses seven electrons D) Loses one electron E) Loses two electrons

E

What is the classification for this unbalanced reaction? Fe + HCl --------> FeCl3 + H2 A) dehydration B) Combination C) Decomposition D) Single replacement E) Double replacement

E

What is the coefficient for oxygen in the balanced equation? A) 2 B) 4 C) 5 D) 6 E) 8

E

What is the correct formula for iron(III) sulfide? A) Fe2S2 B) Fe2S C) FeS D) FeS2 E) Fe2S3

E

What is the element with the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^6 A) Be B) Cl C) F D) S E) Ar

E

What is the molar mass of Mg3(PO4)2, a substance formerly used in medicine as an antacid? A) 71.3 g B) 118 g C) 150. g D) 214 g E) 263 g

E

What is the pressure, in mmHg, of a 4.00 g sample of O2 gas, which has a temperature of 30.0 °C, and a volume of 3000 mL? A) 0.788 mmHg B) 1.04 mmHg C) 78.0 mmHg D) 7880 mmHg E) 788 mmHg

E

What is the symbol for the ion with 19 protons and 18 electrons? A) F+ B) F- C) Ar+ D) K- E) K+

E

What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH? A) 18 mL B) 0.13 mL C) 13 mL D) 120 mL E) 8.0 × 102 mL

E

When 2 moles of Mg3N2 are allowed to react, how many moles of H2O also react? A) 1 mole B) 4 moles C) 6 moles D) 8 moles E) 12 moles

E

Which of the following does not involve change of state? A) melting ice B) freezing water C) vaporization of alcohol D) sblimanation of dry ice E) pouring water into vacuum-insulated bottle

E

Which of the following examples illustrates a number that is correctly rounded to three significant figures? A) 4.05438 grams to 4.054 grams B) 0.03954 grams to 0.040 grams C) 103.692 grams to 103.7 grams D) 109,526 grams to 109 500 grams E) 20.0332 grams to 20.0 grams

E

Which of the following is the smallest unit? (1g = 10dg) A) gram B) milligram C) Kilogram D) decigram E) microgram

E

he name of Al2(SO4)3 is A) aluminum(III)sulfate B) dialuminum trisulfate C) dialuminum sulfate D) dialuminum trisulfide E) aluminum sulfate

E