Thermodynamics Test

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Thermodynamics Test - 38

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Weekly Quiz Competition

Question 1
4 / -1

The formation of water from H₂ (g) and O₂ (g) is an exothermic reaction because

A
H₂(g) and O₂(g) have a higher chemical energy than water

B
H₂(g) and O₂(g) have a lower chemical energy than water

C
H₂(g) and O₂(g) have a higher temperature than water

D
Energy considerations do not arise
Question 2
4 / -1

Which one of the following expresses Q as the heat of combustion ?

A
2H₂ + O₂ → 2H₂O + Q

B
C + 1/2 O₂ → CO + Q

C
CH₄ + 2 O₂ → CO₂ + 2H₂O + Q

D
2C₆H₆ + 15 O₂ → 12 CO₂ + 6H₂O + Q
Question 3
4 / -1

Which one of the following expresses heat of formation of CO₂ ?

A
CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂, ∆H = –a kcal

B
CO + 1/2 O₂ → CO₂ , ∆H = -b kcal

C
C + O₂ → CO₂, ∆H = -c kcal

D
2NaHCO₃ → Na₂CO₃ + H₂O + CO₂, ∆H = +d kcal
Question 4
4 / -1

In which one of the following cases, the heat of neutralization is minimum?

A
Neutralization of NH₄OH with HCl

B
Neutralization of NaOH with CH₃COOH

C
Neutralization of NaOH with HNO₃

D
Neutralization of NH₄OH with CH₃COOH
Question 5
4 / -1

The enthalpy of reaction at constant volume (∆E) is related to the enthalpy of reaction at constant pressure (∆H) as

A
∆H = ∆E − ∆n_g RT

B
∆H = ∆E + ∆n_g RT

C
‒∆H = ‒∆E + ∆n_g RT

D
None of these is correct
Question 6
4 / -1

When 1 mole of H₂O₂ is decomposed by platinum black, the heat evolved is 96.6 kJ. The heat of formation of 1 mole of H₂O₂ is

A
96.6 kJ

B
193.2 kJ

C
386.4 kJ

D
48.3 kJ

Solution
Question 7
4 / -1

The heat of combustion of solid benzoic acid at constant volume is – 321.30 kJ at 27^oC. The heat of combustion at constant pressure is

A
–321.30 – 300 R

B
–321.30 + 300 R

C
–321.30 – 150 R

D
–321.30 + 900 R

Solution
Question 8
4 / -1

A hypothetical reaction, A → 2 B, proceeds through following sequence of steps A → C; ∆H = q₁ , C → D; ∆H = q₂, 1/2 D → B ; ∆H = q₃ . The heat of reactions is:

A
q₁ ‒ q₂ + 2q₃

B
q₁ + q₂ ‒ 2q₃

C
q₁ + q₂ + 2q₃

D
q₁ + 2q₂ ‒ 2q₃
Question 9
4 / -1

The bond energy of H₂ is 436.4 kJ. This means that

A
436.4 kJ of heat is required to break one bond in H₂ molecule to give two atoms of hydrogen

B
436.4 kJ of heat is required to dissociate 6.02 × 10²³ molecules of H₂ to form H-atoms

C
436.4 kJ of heat is required to dissociate 3.01 × 10²³ molecules of H₂ to 6.02 × 10²³ atoms of hydrogen

D
436.4 kJ of electrical energy is required to dissocitate 6.02 × 10²³ molecules of H₂ to form H⁺ and H⁻ ions.
Question 10
4 / -1

If E, R and D represent respectively the tendency for minimum energy, tendency for maximum randomness and overall driving force and arrows represent the direction and magnitude of these tendencies, which one of the following applies correctly to the reaction 2HgO (s) → 2 Hg (l) + O₂ (g) ?

A

B

C

D

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Thermodynamics Test - 38

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Thermodynamics Test - 38

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Question 1

H2(g) and O2(g) have a higher chemical energy than water

H2(g) and O2(g) have a lower chemical energy than water

H2(g) and O2(g) have a higher temperature than water

Energy considerations do not arise

Question 2

2H2 + O2 → 2H2O + Q

C + 1/2 O2 → CO + Q

CH4 + 2 O2 → CO2 + 2H2O + Q

2C6H6 + 15 O2 → 12 CO2 + 6H2O + Q

Question 3

CaCO3 + 2HCl → CaCl2 + H2O + CO2, ∆H = –a kcal

CO + 1/2 O2 → CO2 , ∆H = -b kcal

C + O2 → CO2, ∆H = -c kcal

2NaHCO3 → Na2CO3 + H2O + CO2, ∆H = +d kcal

Question 4

Neutralization of NH4OH with HCl

Neutralization of NaOH with CH3COOH

Neutralization of NaOH with HNO3

Neutralization of NH4OH with CH3COOH

Question 5

∆H = ∆E − ∆ng RT

∆H = ∆E + ∆ng RT

‒∆H = ‒∆E + ∆ng RT

None of these is correct

Question 6

96.6 kJ

193.2 kJ

386.4 kJ

48.3 kJ

Solution

Question 7

–321.30 – 300 R

–321.30 + 300 R

–321.30 – 150 R

–321.30 + 900 R

Solution

Question 8

q1 ‒ q2 + 2q3

q1 + q2 ‒ 2q3

q1 + q2 + 2q3

q1 + 2q2 ‒ 2q3

Question 9

436.4 kJ of heat is required to break one bond in H2 molecule to give two atoms of hydrogen

436.4 kJ of heat is required to dissociate 6.02 × 1023 molecules of H2 to form H-atoms

436.4 kJ of heat is required to dissociate 3.01 × 1023 molecules of H2 to 6.02 × 1023 atoms of hydrogen

436.4 kJ of electrical energy is required to dissocitate 6.02 × 1023 molecules of H2 to form H+ and H− ions.

Question 10

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H₂(g) and O₂(g) have a higher chemical energy than water

H₂(g) and O₂(g) have a lower chemical energy than water

H₂(g) and O₂(g) have a higher temperature than water

2H₂ + O₂ → 2H₂O + Q

C + 1/2 O₂ → CO + Q

CH₄ + 2 O₂ → CO₂ + 2H₂O + Q

2C₆H₆ + 15 O₂ → 12 CO₂ + 6H₂O + Q

CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂, ∆H = –a kcal

CO + 1/2 O₂ → CO₂ , ∆H = -b kcal

C + O₂ → CO₂, ∆H = -c kcal

2NaHCO₃ → Na₂CO₃ + H₂O + CO₂, ∆H = +d kcal

Neutralization of NH₄OH with HCl

Neutralization of NaOH with CH₃COOH

Neutralization of NaOH with HNO₃

Neutralization of NH₄OH with CH₃COOH

∆H = ∆E − ∆n_g RT

∆H = ∆E + ∆n_g RT

‒∆H = ‒∆E + ∆n_g RT

q₁ ‒ q₂ + 2q₃

q₁ + q₂ ‒ 2q₃

q₁ + q₂ + 2q₃

q₁ + 2q₂ ‒ 2q₃

436.4 kJ of heat is required to break one bond in H₂ molecule to give two atoms of hydrogen

436.4 kJ of heat is required to dissociate 6.02 × 10²³ molecules of H₂ to form H-atoms

436.4 kJ of heat is required to dissociate 3.01 × 10²³ molecules of H₂ to 6.02 × 10²³ atoms of hydrogen

436.4 kJ of electrical energy is required to dissocitate 6.02 × 10²³ molecules of H₂ to form H⁺ and H⁻ ions.