Which of the following compounds will behave least like an ideal gas at low temperatures

a) He b) SO2 c) H2 d) N2 e) F2

Table of Contents Show

• a) He b) SO2 c) H2 d) N2 e) F2
• Leave a Comment
• Why do gases behave less ideally at low temperature?
• How do you determine which gas behaves least ideally?
• Which gas behaves less ideally ch4 or so2?
• Do gases behave ideally at low temperature?

Sulfur dioxide should be the least volatile, have the greatest intermolecular interaction, and thus its behaviour is LEAST like the ideal.

As a scientist you should check the boiling points of the gases. Clearly, the one that is most involatile is least like the ideal. Given that sulfur dioxide has the most electrons, there is greater opportunity for Van der Waals interactions, and deviation from ideality.

1. JEE Questions
2. Which Of The Following Compounds Will Behave Least Like An Ideal Gas At Low Temperature

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Classification and Properties of Matter

In chemistry and physics, matter is any substance that has mass and takes up space by having volume. All everyday objects that can be touched are ultimately composed of atoms, which are made up of interacting subatomic particles, and in everyday as well as scientific usage, "matter" generally includes atoms and anything made up of them, and any particles and objects that act as if they have both rest mass and volume. However it does not include massless particles such as photons, or other energy phenomena or waves such as light or sound. Matter exists in various states (known as phases) that are defined by various physical properties, such as state of matter, phase, shape, and density. The Standard Model of particle physics and the general theory of relativity describe fundamental particles and the fundamental forces acting between them that control the structure and dynamics of matter.

Which of the gases in the graph below has the largest molar mass?

Look at Quiz

D

Calculate the root mean square velocity of nitrogen molecules at 25°C.

A) 729 m/s

B) 515 m/s

C) 149 m/s

D) 297 m/s

B

Which of the following statements is TRUE?

A) At a given temperature, lighter gas particles travel more slowly than heavier gas particles.

B) The smaller a gas particle, the slower it will effuse

C) The higher the temperature, the lower the average kinetic energy of the sample.

D) At low temperatures, intermolecular forces become important and the pressure of a gas will be lower than predicted by the ideal gas law.

E) None of the above statements are true.

D

If NO and NH3 are allowed to effuse through a porous membrane under identical conditions, the rate of effusion for NH3 will be ________ times that of NO .

A) 0.57

B) 0.75

C) 1.3

D) 1.8

C

Rank the following in order of decreasing rate of effusion.

F2 SF6 He Ar

A) SF6 > Ar > F2 > He

B) Ar > He > SF6 > F2

C) F2 > Ar > He > SF6

D) He > F2 > Ar > SF6

E) He > F2 > SF6 > Ar

D

Which of the following compounds will behave LEAST like an ideal gas at low temperatures?

A) He

B) SO2

C) H2

D) N2

E) F2

B

Energy that is associated with the relative positions of electrons and nuclei in atoms and molecules is called

A) kinetic energy

B) thermal energy

C) potential energy

D) chemical energy

D

Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as gaining heat from the surroundings?

A) q = +, w = -

B) q = -, w = +

C) q = +, w = +

D) q = -, w = -

E) None of these represent the system referenced above.

A

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?

A) 50.0 g Al, CAl = 0.903 J/g°C

B) 50.0 g Cu, CCu = 0.385 J/g°C

C) 25.0 g granite, Cgranite = 0.79 J/g°C

D) 25.0 g Au, CAu = 0.128 J/g°C

E) 25.0 g Ag, CAg = 0.235 J/g°C

A

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter.

4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 NO2(g)

ΔH°rxn = -1.28 x 104 kJ

A) 97.3 kJ/°C

B) 38.9 kJ/°C

C) 5.94 kJ/°C

D) 6.84 kJ/°C

E) 12.8 kJ/°C

D

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 14.25 kJ/°C. If the initial temperature was 32.9°C, use the information below to determine the value of the final temperature of the calorimeter.

4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 NO2(g)

ΔH°rxn = -1.28 x 104 kJ

A) 257°C

B) 46.6°C

C) 48.7°C

D) 41.9°C

E) 931°C

C

How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below?

Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ

A) 753 kJ

B) 1.51 x 103 kJ

C) 4.20 x 103 kJ

D) 482 kJ

E) 241 kJ

A

According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g/mol.

B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) ΔH°rxn = -1396 kJ

A) 1640 kJ

B) 238 kJ

C) 1430 kJ

D) 3070 kJ

E) 429 kJ

B

A student is preparing to perform a series of calorimetry experiments. She first wishes to determine the calorimeter constant (Ccal) for her coffee cup calorimeter. She pours a 50.0 mL sample of water at 345 K into the calorimeter containing a 50.0 mL sample of water at 298 K. She carefully records the final temperature of the water as 317 K. What is the value of Ccal for the calorimeter?

A) 19 J/K

B) 28 J/K

C) 99 J/K

D) 21 J/K

E) 76 J/K

C

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction:

4 SO3(g) → 4 S(s) + 6 O2(g) ΔH°rxn = ?

Given:

SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ

2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -197.8 kJ

A) -494.6 kJ

B) -692.4 kJ

C) -791.4 kJ

D) 1583 kJ

E) -293.0 kJ

D

Choose the thermochemical equation that illustrates ΔH°f for Li2SO4.

A) 2 Li+(aq) + SO42-(aq) → Li2SO4(aq)

B) 2 Li(s) + 1/8 S8(s, rhombic) + 2 O2(g) → Li2SO4(s)

C) Li2SO4(aq) → 2 Li+(aq) + SO42-(aq)

D) 8 Li2SO4(s) → 16 Li(s) + S8(s, rhombic) + 16 O2(g)

E) 16 Li(s) + S8(s, rhombic) + 16 O2(g) → 8 Li2SO4(s)

B

Use the information provided to determine ΔH°rxn for the following reaction:

ΔH°f (kJ/mol) CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) ΔH°rxn = ?

CH4(g) -75

CCl4(g) -96

HCl(g) -92

A) -389 kJ

B) -113 kJ

C) +113 kJ

D) -71 kJ

E) +79 kJ

A

Use the information provided to determine ΔH°rxn for the following reaction:

ΔH°f (kJ/mol) 3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g) ΔH°rxn = ?

Fe2O3(s) -824

Fe3O4(s) -1118

CO(g) -111

CO2(g) -394

A) +277 kJ

B) -577 kJ

C) -47 kJ

D) +144 kJ

E) -111 kJ

C

On the electromagnetic spectrum, visible light is immediately between two other wavelengths. Name them.

A) infrared and x-ray

B) radio and microwave

C) gamma ray and ultraviolet

D) microwave and x-ray

E) infrared and ultraviolet

E

When a wave encounters an obstacle or a slit that is comparable in size to its wavelength, it bends around it. This characteristic is called ________.

A) destructive interference

B) diffraction

C) constructive interference

D) effusion

E) amplitude

B

Which of the following statements is TRUE?

A) The emission spectrum of a particular element is always the same and can be used to identify the element.

B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus.

C) The uncertainty principle states that we can never know both the exact location and speed of an electron.

D) An orbital is the volume in which we are most likely to find an electron.

E) All of the above are true.

E

Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of 1.33 × 10-35 m.

A) 8.81 m/s

B) 12.3 m/s

C) 2.21 m/s

D) 4.98 m/s

E) 6.44 m/s

D

How many orbitals are contained in the third principal level (n = 3) of a given atom?

A) 9

B) 3

C) 18

D) 7

E) 5

A

Describe the shape of a p orbital.

A) spherical

B) dumbbell shaped

C) three balls

D) four balls

E) eight balls

B

What is the maximum number of p orbitals that are possible in the same shell?

A) 1

B) 3

C) 7

D) 5

E) 9

B

When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as

A) Pauli exclusion principle

B) Hund's rule

C) Aufbau principle

D) Heisenberg uncertainty principle

E) None of the above

B

Valence Electron Diagram Look At Quiz

A

Give the ground state electron configuration for Cd.

A) [Kr]5s25d10

B) [Kr]5s24d105p2

C) [Kr]4d10

D) [Kr]5s24d8

E) [Kr]5s24d10

E

Place the following elements in order of increasing atomic radius.

P Ba Cl

A) Ba < P < Cl

B) P < Cl < Ba

C) Cl < P < Ba

D) Cl < Ba < P

E) Ba < Cl < P

C

Place the following in order of decreasing radius.

Te2⁻ F⁻ O2⁻

A) F⁻ > O2⁻ > Te2⁻

B) F⁻ > Te2⁻ > O2⁻

C) Te2⁻ > O2⁻ > F⁻

D) Te2⁻ > F⁻ > O2⁻

E) O2⁻ > F⁻ > Te2⁻

C

Which reaction below represents the second ionization of Sr?

A) Sr(g) → Sr⁺(g) + e⁻

B) Sr2⁺(g) + e⁻ → Sr⁺(g)

C) Sr⁺(g) + e⁻ → Sr(g)

D) Sr⁻(g) + e⁻ → Sr2⁻(g)

E) Sr⁺(g) → Sr2⁺(g) + e⁻

E

Place the following in order of increasing IE1.

K Ca Rb

A) Ca < K < Rb

B) Rb < Ca < K

C) Ca < Rb < K

D) Rb < K < Ca

E) K < Ca < Rb

D

Give the ground state electron configuration for Rb⁺.

A) [Ar]4s24p6

B) [Kr]5s1

C) [Ar]4s23d104p6

D) [Kr]5s2

E) [Kr]5s24d2

C

Which reaction below represents the second electron affinity of S?

A) S(g) + e⁻ → S⁻(g)

B) S⁻(g) + e⁻ → S2⁻(g)

C) S(g) → S⁺(g) + e⁻

D) S⁻(g) → S(g) + e⁻

E) S2⁻(g) → S⁻(g) + e⁻

B

Identify the most reactive alkali metal with water.

A) Cs

B) Rb

C) K

D) Na

E) Li

A

Why do gases behave less ideally at low temperature?

How do you determine which gas behaves least ideally?

Which gas behaves less ideally ch4 or so2?

Do gases behave ideally at low temperature?