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3721. Which of the equations shows twice the enthalpy change of neutralization as the following equation: HCl + NaOH → NaCl + H₂O

NH₄Cl + NaOH → NaCl + H₂O + NH₃
MgCO₃ + 2HCl → MgCl₂ + CO₂ + H₂O
KOH + HCl → KCl + H₂O
H₂SO₄ + Mg(OH)₂ → MgSO₄ + 2H₂O

3722. The given diagram shows the enthalpy changes during a chemical reaction. The diagram represents:

A non-spontaneous process
An isothermic process
An endothermic reaction
An exothermic reaction

3723. Which enthalpy change is relevant in the following process: Na(s) → Na(g) ΔH = ?

Enthalpy of atomization
Enthalpy of vaporization
Enthalpy of fusion
Enthalpy of formation

3724. The enthalpy change when one mole of water is formed by the reaction of acid with an alkali under standard conditions is known as:

Enthalpy of formation
Enthalpy of reaction
Enthalpy of combustion
Enthalpy of neutralization

3725. The thermal energy at constant pressure is called:

Enthalpy
Internal energy
Heat capacity
Work done

3726. Which of the following information do we obtain from the lattice energy?

It helps while explaining the structure of the ionic compound
It explains bonding in the covalent compound
It explains properties of the metallic compound
It explains the structure of molecular compound

3727. For an endothermic reaction, H represents the enthalpy of reaction. The minimum value for the energy for activation will be:

Equal to ΔH
More than ΔH
Less than ΔH
Zero

3728. The specific heat of water is:

4.2 J/gK
9.82 J/g/°C
6.04 J/g/°C
8.47 J/g/°C

3729. The thermal energy at constant pressure is called:

Enthalpy
Internal energy
Heat capacity
Work capacity

3730. Enthalpy change of combustion is exothermic because:

Energy released in bond breaking is greater
Energy released in bond making is greater
Energy absorbed in bond breaking is greater
Energy absorbed in bond making is greater

3731. Born–Haber cycle is used to determine the lattice energy of ionic compounds. It is the application of:

Henry's law
Le-Chatelier's principle
Hess's law
Common Ion Effect

3732. All of the following steps are used to calculate the lattice energy in Born–Haber cycle except:

Atomizing the metal
Ionizing the metal
Deionize the metal
Ionize non-metal

3733. Reaction taking place in one step or in several steps have same ΔH. It is the statement of:

Lussac's law of combining volume
Hess's law
Boyle's law
Charles's law

3734. Born–Haber cycle is used to calculate the lattice energy of which compound?

RbBr
PbS
SO₂
NH₃

3735. ΔH can be measured indirectly by applying:

Avogadro's law
Gas's law
Faraday's law
Hess's law

3736. Born–Haber cycle is used to determine the lattice energies of:

Molecular solids
Metallic solids
Ionic solids
Covalent solids

3737. The lattice energy is also called:

Energy of affinity
Bond energy
Crystal energy
Potential energy

3738. Energy change in a cyclic process is always equal to zero. This is the statement of:

Hess's law
Law of conservation of energy
Henry's law
Charles's law

3739. The following equation represents which energy change? Mg²⁺(g) + O²⁻(g) → MgO(s)

Atomization
Lattice energy
Neutralization
Solution

3740. For an equilibrium reaction: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) The forward reaction is exothermic, increase in temperature shifts the equilibrium position toward left because:

The concentrations of SO₂ and O₂ decrease and concentration of SO₃ increases as the temperature increases
The concentration of SO₂ and O₂ increases and concentration of SO₃ decreases as the temperature increases
The concentrations of SO₂ and O₂ increase and concentrations of SO₃ stays same as the temperature increases
The concentrations of SO₂, SO₃ and O₂ increase as the temperature increases