Thermodynamics Test

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Thermodynamics Test - 3

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Weekly Quiz Competition

Question 1
1 / -0

Consider the reaction: 2C + O₂ → 2CO₂, ΔH = - 395.5 kJ/mol. Which of the following statements is/are correct for this reaction?

A
Bond is formed between products.

B
The reaction is exothermic.

C
The reaction needs no initiation.

D
All of the above

Solution

Since the reaction involves the release of energy, so it is an exothermic reaction.
Question 2
1 / -0

Which of the following reactions corresponds to the definition of enthalpy of formation?

A
H₂(g) + 1/2 O₂(g) → H₂O(l)

B
H₂(g) + 1/2 O₂(s) → H₂O(l)

C
H₂(g) + 1/2 O₂(l) → H₂O(l)

D
2H₂(g) + O₂(g) → 2H₂O(l)

Solution

This option is correct because heat of formation is the heat change when one mole of a substance is formed from its constituent elements in gaseous state and in the given option, both the reactants are in gaseous state.
Question 3
1 / -0

The amount of heat liberated when 1 mole of a substance at 298K and 1 bar pressure is completely burnt in the presence of oxygen is known as

A
standard enthalpy of combustion

B
specific heat capacity

C
enthalpy of atomisation

D
molar heat capacity

Solution

Standard enthalpy of combustion is defined as the enthalpy change when one mole of a compound is completely burnt in oxygen with all the reactants and products in their standard state under standard conditions (298K and 1 bar pressure).
Question 4
1 / -0

Bond energy of hydrogen gas is - 433 kJ. What is the bond dissociation energy of 0.5 mole of hydrogen gas?

A
- 433 kJ

B
+ 433 kJ

C
- 216.5 kJ

D
216.5 kJ

Solution

Bond dissociation energy = - Bond formation energy
Bond energy of hydrogen gas is - 433 kJ. mol^-1.
Bond energy for half mole of hydrogen gas is - 216.5 kJ.
Bond dissociation energy of 0.5 mole of hydrogen gas = 216.5 kJ
Question 5
1 / -0

For the reaction 2H₂ + O₂ →2H₂O, ΔH = -571 kJ, bond energy of H - H = 435 kJ/mol and that of O - O = 498 kJ/mol. Calculate the average bond energy (in kJ/mol) ofO - H bond using this data.

A
484

B
-484

C
271

D
-271

Solution

Using the formula,
ΔH = Energy of bonds broken - Energy of bonds formedLet the average B.E of O-H bonds be x kJ mol^-1.
-571 = (2 × 435) + 498 - (4x)x = 484.75 kJ mol^-1
Question 6
1 / -0

Hess's Law deals with

A
change in heat

B
rate of reaction

C
equilibrium constant

D
influence of pressure on volume of a gas

Solution

Hess' Law states that the heat evolved or absorbed in a chemical process is the same whether the process takes place in one or in several steps. This is also known as the law of constant heat summation.

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Thermodynamics Test - 3

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Thermodynamics Test - 3

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Question 1

Bond is formed between products.

The reaction is exothermic.

The reaction needs no initiation.

All of the above

Solution

Question 2

H2(g) + 1/2 O2(g) → H2O(l)

H2(g) + 1/2 O2(s) → H2O(l)

H2(g) + 1/2 O2(l) → H2O(l)

2H2(g) + O2(g) → 2H2O(l)

Solution

Question 3

standard enthalpy of combustion

specific heat capacity

enthalpy of atomisation

molar heat capacity

Solution

Question 4

- 433 kJ

+ 433 kJ

- 216.5 kJ

216.5 kJ

Solution

Question 5

484

-484

271

-271

Solution

Question 6

change in heat

rate of reaction

equilibrium constant

influence of pressure on volume of a gas

Solution

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H₂(g) + 1/2 O₂(g) → H₂O(l)

H₂(g) + 1/2 O₂(s) → H₂O(l)

H₂(g) + 1/2 O₂(l) → H₂O(l)

2H₂(g) + O₂(g) → 2H₂O(l)