CHM 1045 Final

What a stable compound can two elements Ca and N form?

Ca3N2

Which of the following has the lowest solubility in water? CaCO3 K3PO4 LiOH AgNO3

CaCO3

Which of the following compounds requires the most energy to convert one mole of the solid into separate ions? CaO K2O K2S CaS

CaO

What is the name of polyatomic ion ClO2- ?

Chlorite

Water is a(n)? - mixture - compound - alloy - element

Compound

The density of a certain gaseous hydrocarbon (containing only C and H) is 1.25 g/L at standard temperature and pressure (STP). What is the compound? (Gas constant, R = 0.08206 L atm K−1 mol−1)

C₂H₄

A compound, containing C, H, and Cl, has a molar mass of 99 g/mol. Analysis of a sample shows that it contains 24.3% C, and 71.6% Cl. What is its molecular formula? The atomic masses of C, H, and Cl are 16 amu, 1 amu, and 35.5 amu, respectively.

C₂H₄Cl₂

The density of a certain gaseous hydrocarbon (containing only C and H) is 1.34 g/L at standard temperature and pressure (STP). What is the compound? (Gas constant, R = 0.08206 L atm K−1 mol−1)

C₂H₆

Which of the following could NOT be found in a hazard diamond? - reactivity - density - radioactive - fire hazard

Density

When 23 g of Sodium (molar mass 23 g/mol) and 30 g of diatomic chlorine (molar mass 71 g/mol) combine to form sodium chloride (NaCl), which of the following statement is correct? Diatomic chlorine is the limiting reactant Neither is the limiting reactant Sodium is the limiting reactant None of above

Diatomic chlorine is the limiting reactant

Which of the following is a compound? - Gasoline - Dry ice - Air - Nitrogen

Dry ice

Which of the following is an extensive property of a substance? Density Enthalpy Temperature Specific Heat Capacity

Enthalpy

Which of the following has the most negative electron affinity value? (greatest affinity to electrons) F Li C B

F

Which of the following has the longest wavelength? FM Radio Infrared light X-Rays UV light

FM Radio

Which of the following do exist as individual atoms? - Hydrogen - Oxygen - Sulfur - Gold

Gold

Which of the following experiment was performed to discover the nucleus? - Aluminum foil diffraction experiment - Oil drop experiment - Cathode ray tube experiment - Gold foil scattering experiment

Gold foil scattering experiment

Which of the following about the bond strength comparison is NOT correct? C-Cl is stronger than C-Br H-S is stronger than H-Cl N=N is stronger than N-N N-F is stronger than N-P

H-S is stronger than H-Cl

Which of the following compounds is NOT an ionic compound? BeO KClO4 (NH4)2CO3 H2S

H2S

What is the formula for nitrous acid?

HNO3

Which of the following is an extensive property? - heat - density - boiling point - temperature

Heat

Under which set of conditions does a real gas behave most like an ideal gas?

High temperature, low pressure

What will happen to the average kinetic energy of idea gas molecules when the pressure of the gas is increased by increasing the temperature at constant volume.

Increases

Who performed experiments to find out the charge-to-mass ratio of an electron for the first time?

J. J. Thomson

What is the chemical formula of potassium phosphate?

K2HPO4

How many carbon dioxide molecules are produced when 32 g of methane (CH4, Molar Mass 16 g/mol) is completely combusted with oxygen in air?

1.2 x 10^24

The end point in a titration of a 500 mL sample of aqueous HCl was reached by addition of 1 L of 0.4 M Ca(OH)2 titant. What is the molarity of the HCl?

1.6 M

What is the charge of an electron?

1.6 × 10z6-19 C

What is the number of electrons in an ion 27Al3+ ?

10

Which of the following is the highest pressure? 10 Pa 10 torr 10 cm Hg 10 N/cm2

10 N/cm2

A material with a density of 10 g/mL has a volume of 10 L, what is the mass of this material in Kg?

100 Kg

A piece of metal alloy with a specific heat of 0.5 J / ( g ⋅ oC ) is cooled down from 150 oC to 50 oC to release 5 KJ of heat. What is the mass of this piece of metal alloy?

100 g

Methanol, CH3OH, could decompose into carbon monoxide, CO, and hydrogen, H2. What is the approximate enthalpy change of this reaction? (Bond Energies: CO, 1080 KJ/mol; H-H, 436 KJ/mol; C-H, 415 KJ/mol; C-O, 350 KJ/mol; O-H, 464 KJ/mol)

107 KJ

What is 50 degrees C converted into F?

122 F

What is the number of neutrons in an ion 25Mg2+ ?

13

A balloon filled with Hydrogen gas (2g/mol) is found to take 4 hours to deflate to 50% of its original volume. How long will it take for an identical balloon filled with the same volume of Oxygen gas (32 g/mol) to decrease its volume by 50%?

16 Hours

What is the formula mass of Calcium Nitrate? The atomic masses of Ca, N, and O are 40 amu, 14 amu, and 16 amu, respectively.

164 amu

What is the molecular mass of Aspirin, ? The atomic masses of C, H, and O are 12 amu, 1 amu, and 16 amu, respectively.

180 amu

What is the electron configuration of Cl?

1s^2 2s^2 2p^6 3s^2 3p^5

What is the volume of a gas weighted 8 Kg with a density of 4 g/L? 32 m3 2 m3 2 L 32 L

2 m^3

How many water molecules are produced when 1 mol of propane (C3H8) is completely combusted with oxygen (O2) in air ?

2.4 x 10^24

What is the pressure of the gas sample in the following mercury manometer? (picture shows closed end, 26.4 cm)

264 mm Hg

What mass of potassium hydroxide (molar mass 56 g/mol) would be required to react with calcium chloride to produce 18.5 g calcium hydroxide (molar mass 74 g/mol) in a reaction?

28 g

At the same temperature and pressure, which of the following gases diffuse fastest? CO CH4 O2 C2H2

CH4

Which of the following is NOT a part of basic laws of stoichiometry - Law of conservation of mass - Law of definite composition - Law of mass energy conversion - Law of multiple proportions.

Law of mass energy conversion

Which of the following is NOT supposed to be in a hand sanitizer? - Methanol - Ethanol - Isopropanol - Propanol

Methanol

What a stable compound can two elements Mg and P form?

Mg3P2

Which of the following is ionic? IBr MgO H2S NF3

MgO

Which of the following has the lowest energy? X-ray Microwave radiation Infrared light Blue light

Microwave radiation

Which of the following involves an endothermic process? Mixing ammonium nitrate with water Starting a gas oven Lighting a match Ice cubes freezing

Mixing ammonium nitrate with water

Which of the following statements is correct? Most ionic and covalent compounds are good conductors of electricity. Both electron affinity and electronegativity could be measured experimentally. Most ionic and covalent compounds are electrically neutral. Most ionic and covalent compounds are soluble in water.

Most ionic and covalent compounds are electrically neutral.

Which of the following compound does not have resonance structures? N2O SO2 HCO3- NO2-

N2O

What is the empirical formula for a compound with 26% (percentage composition) Nitrogen and 74% Oxygen? The atomic masses of N and O are 14 and 16, respectively.

N2O5

Which of the following has the highest solubility in water? Mg(OH)2 PbS NH4Br BaSO4

NH4Br

Which of the following contains a double bond? Cl2 NO- N2 C2H2

NO-

Which of the following has the largest atomic radius? O F Na Li

Na

A molecular equation, Na2CO3 + Ba(OH)2 ⟶ NaOH + BaCO3 could be simplified into a net ionic equation. Which of the following is NOT a part of the net ionic equation? Ba2+ (aq) CO32- (aq) BaCO3 (s) Na+ (aq)

Na+ (aq)

What is the chemical formula of sodium bicarbonate?

NaHCO3

Which of the following is NOT an acid-base reaction? NH3 (aq) + H2O (l) ↔ NH4+(aq) +OH-(aq) HCl (aq) + H2O (l) → Cl- (aq) +H3O+(aq) CH3COOH (aq) + H2O (aq) ↔ CH3COO-(aq) +H3O+(aq) NaOH(s) → Na+(aq) + OH-

NaOH(s) → Na+(aq) + OH-

Which of the following is not an isoelectronic species in reference to the other three? Ca2+ Cl- Ne P3-

Ne

Which of the following is a covalent compound? SiC MgS Al2O3 CaO

SiC

Which of the following is an intensive property of a substance? Kinetic Energy Enthalpy Specific heat Potential Energy

Specific heat

Which of the following involves an exothermic process? Melting ice cubes Starting a gas oven Instant cold pack Mixing water and ammonium nitrate

Starting a gas oven

Which of the following is NOT an extensive property? - Volume - Heat - Mass - Temperature

Temperature

Which of the following has the same oxidation state as S in SO2? N in N2O5 Ti in TiCl4 P in H3PO4 S in H2SO4

Ti in TiCl4

Which of the following is a physical change? - Iron rusting - Banana aging - Water boiling - Cooking red meat

Water boiling

Which of the following is NOT a chemical change? - wax burning - wax melting - banana aging - iron rusting

Wax melting

What is the electron configuration of Cl+ ?

[Ne]3s²3p⁴

What is the shape of a p orbital?

dumbbell

Is mass an intensive or extensive property?

extensive

Which of the following is NOT an SI unit? - mol/L - g/mL - g/Gal - K/s

g/Gal

Which of the following is NOT a SI base unit? - kmol/L - g/mL - km/s - lb/L

lb/L

How many spikes does a COVID virus have?

~ 90

What is the molarity of 49.0 g of phosphoric acid, H3PO4 (molecular mass 98 g/mol), in 500 mL of solution?

1.0 M

Which of the following is equal to - 40 oC? - 40 K - 40 F 313.15 K 233.15 F

- 40 F

What is the enthalpy of combustion of propane, C3H8(g), for the formation of H2O(g) and CO2(g), from the following data? C(s) + O2(g) ⟶ CO2 (g) ΔHfo = -394 KJ/mol H2(g) + 1/2 O2(g) ⟶ H2O (g) ΔHfo = -242 KJ/mol 3C(s) + 4H2(g) ⟶ C3H8 (g) ΔHfo = -104 KJ/mol

-2046 KJ mol^-1

"What is ΔH298 for the process, 3Co (s) + 2O2 (g) →Co3O4 (s) from the following data? Co(s) + 1/2 O2(g) →CoO (s) ΔH298 = -237.9 KJ 3CoO (s) + 1/2 O2(g) →Co3O4 (g) ΔH298 = -177.5 KJ

-891.2 KJ

What is the formal charge of P in PO3^3-?

0

What is the molarity of the diluted solution, when 25 mL of a 0.4 M solution of C12H22O11 is diluted to 100.0 mL?

0.1 M

A throat spray is 1.41 % by mass phenol, C6H5OH (Molecular Mass 94 amu) in water. If the solution has a density of 1 Kg/L, what is the molarity of the solution?

0.15 M

A piece of metal weighs at around 0.2 kg. When the metal piece is heated to have its temperature increase from 20 oC to 60 oC, it absorbs 2000 J of heat. What is the specific heat of this metal?

0.25 J/g oC

What is the number of moles of 14.5 g Butane (C4H10)? The atomic masses of C and H are 12 amu and 1amu, respectively.

0.25 mol

The end point in a titration of a 1 L sample of aqueous H2SO4 was reached by addition of 500 mL of 2 M NaOH titrant. What is the molarity of H2SO4?

0.5 M

An unknown Boron sample (Z = 5) was found to contain two isotopes 10B and 12B, and measured to have an atomic mass of 10.8 amu, what is the fraction of 10B in the sample?

0.6

An unknown carbon sample (Z = 6) was found to contain two isotopes 12C and 14C, and measured to have an atomic mass of 12.8 amu, what is the fraction of 12C in the sample?

0.6

Which of the following is NOT an acid-base reaction? NH3 (aq) + H2O (l) ⟶NH4+(aq) +OH-(aq) 2Na(s) + 2HCl (aq) ⟶ 2NaCl(aq) + H2(g) HCl(aq) + H2O (l) ⟶Cl- (aq) +H3O+(aq) Al(OH)3(aq) + 3HCl (aq) ⟶ AlCl3(aq) + 3H2O(l)

2Na(s) + 2HCl (aq) ⟶ 2NaCl(aq) + H2(g)

What is the subshell, in which electrons are found to have quantum numbers, n = 2, l = 1?

2p

Consider a large number of hydrogen atoms with electrons randomly distributed in the n = 1, 2, and 3 orbits. How many different wavelengths of light are emitted by these atoms as the electrons fall into lower-energy orbitals?

3

How many significant figures are contained in 0.0170 g/mL

3

If a shell contains a maximum of 18 electrons, what is the principal quantum number?

3

When the reaction, solid aluminum metal (Al) reacting with oxygen gas (O2) to form solid aluminum oxide (Al2O3), is balanced, what is the coefficient for oxygen gas?

3

An FM radio station broadcasts at a frequency of 90 MHz (9.0 x 107 s-1). What is the wavelength of these radio waves in meters?

3.33 m

An FM radio station broadcasts at a frequency of 90 MHz. What is the wavelength of these radio waves in meters?

3.33 m

A LED emits light with a wavelength of 530 nm. What is the energy of the photon being emitted? (Planck's constant: h = 6.626 × 10-34 J s)

3.75 x 10^-19 J

A 50 g piece of metal alloy was heated to 100 o C and then dropped into a beaker containing 70 g of water at 25 oC. The specific heat capacities of this metal alloy and water are 0.418 and 4.18 J/(g⋅oC) respectively. These systems are isolated and maintained at the constant volume condition. What is the final temperature, when the water and the metal reach their thermal equilibrium?

30 oC

A piece of metal (100 g, specific heat of 0.42 J / ( g ⋅ oC) ) at 220 oC was dropped into a beaker containing 190 g of water (specific heat capacity of 4.2 J / ( g ⋅ oC ) ) at 20.0 oC. The system is isolated and maintained at the constant volume condition. What is the final temperature?

30°C

Automotive air bags inflate when a sample of sodium azide, NaN3 (molar mass 65 g/mol and density 1.85 g/cm³), is very rapidly decomposed to sodium and nitrogen gas. What volume of sodium azide is required to produce 42 grams of nitrogen gas (molar mass 28 g/mol)?

35.2 cm3

When the half-reaction, H2O(l) → O2 (g) (in acidic solution), is balanced, how many electrons need to be added in the product side?

4

What is the total volume of the CO2(g) and H2O(g) at 819 °C and 0.5 atm produced by the combustion of 1.00 L of C2H6(g) measured at STP?

40 L

What is the most probable molecular speed of Oxygen gas at room temperature (22 C) and one atmosphere pressure?

400 m/s

What mass of sodium hydroxide (NaOH, molar mass 40 g/mol) would be required to react with magnesium chloride (MgCl2) to produce 32 g magnesium hydroxide (molar mass 58.3 g/mol) in a reaction?

44 g

An LED emits a photon with an energy of 2.5 eV. What is the wavelength of the photon being emitted? (Planck's constant: h = 6.626 × 10-34 J⋅s and 1 eV = 1.602 × 10-19 J)

496 nm

What is the subshell, in which electrons are found to have quantum numbers, n = 4, l = 2?

4d

When the equation, Zn (s) + NO3-(aq)→ Zn2+ (aq) + N2(g) (in acid) , is balanced according to the half-reaction method, what is the coefficient for Zn2+?

5

What is the heat capacity of 630 g Aluminum metal (specific heat 0.9 J / ( g ⋅ °C ) )? 700 J / °C 567 °C / J 700 °C / J 567 J / °C

567 J / °C

When the half-reaction, Cl- (aq) ⟶ClO3- (aq) (in basic solution), is balanced, how many electrons need to be added in the product side?

6

What is the mass of the solute in 500 mL of 8.3 × 10-2 M KI (molar mass 166 g/mol)?

6.9 g

How big is the Covid virus?

60-140 nm

Automotive air bags inflate when a sample of sodium azide, NaN3 (molar mass 65 g/mol), is very rapidly decomposed to sodium and nitrogen gas. What mass of sodium azide is required to produce 33.6 L of nitrogen gas (molar mass 28 g/mol) with a density of 1.25 g/L?

65 g

Sucrose (C12H22O11) is a common sugar, with a molar mass of around 342 g/mol. How many Carbon atoms are in 34.2 g sucrose?

7.226 x 10^23

Which of the following is the pressure of standard atmosphere? 76 torr 1 KPa 10 KPa 76 cm Hg

76 cm Hg

What is the number of neutrons in an ion 14C4- ?

8

A cylinder of medical oxygen has a volume of 100 L, and contains O2 at a pressure of 50 atm and a temperature of 27 oC. When the oxygen is regulated to a larger container with a volume of 500L at a temperature of - 23 oC, what is the pressure?

8.33 atm

It takes 40,000 J of energy to raise the temperature of a pan (1.6 Kg) by 50 °C. What is the heat capacity of this pan?

800 J / °C

What is the mass of an electron?

9.1 × 10^28 g

Which of the following is NOT a strong acid? Nitric Acid Sulfuric Acid Acetic Acid Perchloric Acid

Acetic Acid

Which of the following is NOT an oxidation-reduction reaction? Al (OH)3(aq) + 3HCl (l) → AlBr3 (aq) +3H2O(aq) Ca(s) + Br2(l) → CaBr2(s) H2O(g) + C(s) → CO(g) + H2(g) C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(g)

Al (OH)3(aq) + 3HCl (l) → AlBr3 (aq) +3H2O(aq)

Which of the following has the same oxidation state as N in KNO2? S in H2SO4 N in N2O5 P in H3PO4 Al in AlCl3

Al in AlCl3

Which of the following is considered as in macroscopic domain? - a virus - a water molecule - a bacteria - an orange

An orange

Which of the following is NOT an oxidation-reduction reaction? C3H8 + 5O2 ⟶ 3CO2 + 4H2O Ba(OH)2(aq) + 2HF (aq) ⟶ BaF2(aq) + 2H2O(l) H2O + C ⟶ CO + H2 2K (s) + Br2 (l) ⟶ 2KBr (s)

Ba(OH)2(aq) + 2HF (aq) ⟶ BaF2(aq) + 2H2O(l)

Which of the following has the lowest solubility in water? BaSO4 K3PO4 AgNO3 LiOH

BaSO4

Which of the following has the highest first ionization energy? Si B C Al

C

Which of the following has the lowest electronegativity? F C O N

C

When 42 g of Lithium (Li, molar mass ~ 7 g/mol) and 24 g of nitrogen gas (N2, 28 g/mol) combine to form lithium nitride (Li3N), which of the following statement is correct? Nitrogen gas is the limiting reactant Lithium is the limiting reactant Neither is the limiting reactant None of above is correct

Nitrogen gas is the limiting reactant

Solid potassium chlorate, KClO3, decomposes to a solid compound and a gas molecule with stoichiometric coefficients are 2 for KClO3, 2 for the solid compound, and 3 for the gas molecule. Which of the following is one of the products? KO K O2 Cl

O2

Which of the following does not contain a triple bond? O2 CO CN- C2H2

O2

Which of the following is NOT in microscopic domain? - Sea salt dissolved in water - One mole of water molecules - One COVID-19 virus - A quantum dot with 5 nm diameter

One mole of water molecules

Which of the following is NOT one of the four quantum numbers? Magnetic quantum number Principle quantum number Orbital quantum number Angular momentum quantum number

Orbital quantum number

Which of the following is consider as nonmetal? - B - Be - Al - P

P

Which of the following is NOT a part of ideal gas law? n ∝ V V ∝ T P ∝ T P ∝ V

P ∝ V