Thermodynamics - Practice Test (1) - Class 9 MCQ

heat and its transformations to and from other forms of energy

Potential and its transformations to and from other forms of energy

kinetic energy and its transformations to and from other forms of energy

mass and its transformations to and from other forms of energy

the sum of the standard enthalpies of the intermediate reactions into which the overall reaction may be divided at 35^∘C

the sum of the standard enthalpies of the intermediate reactions into which the overall reaction may be divided at the same temperature

the sum of the standard enthalpies of the intermediate reactions into which the overall reaction may be divided at 2 bar

the difference of the standard enthalpies of the intermediate reactions into which the overall reaction may be divided at the same temperature

not possible at any temperature

possible only at low temperature

possible at any temperature

possible at high temperature

NO₂(g) is unstable, but NO(g) is formed

NO(g) is stable, but NO₂(g) is formed

NO(g) is unstable, but NO₂(g) is formed

NO₂ (g) is stable, but NO(g) is formed

ΔG is negative for a spontaneous reaction

ΔG is zero for a reversible reaction

ΔG is positive for a non-spontaneous reaction

ΔG is positive for a spontaneous reaction

the boundaries permit the flow of matter into or out of it

the boundaries prevent the flow of matter out of it

the boundaries prevent the flow of matter into or out of it

the boundaries permit the flow of matter into it

one kg of bonds completely to obtain atoms in the liquid phase

one kg of bonds completely to obtain atoms in the gas phase

One mole of bonds completely to obtain atoms in the gas phase

One mole of bonds completely to obtain atoms in the liquid phase

ΔU = 327 J

ΔU = 367 J

ΔU = 307 J

ΔU = 347 J

28.5 kJ, -28.5 kJ

25.5 kJ, -28.5 kJ

27.0 kJ, -28.5 kJ

30.5 kJ, -28.5 kJ

-776 J

-745 J

-702 J

-797 J

the boundaries prevent the flow of matter into it

the boundaries permit the flow of matter into or out of it

the boundaries prevent the flow of matter into or out of it

the boundaries prevent the flow of matter out of it

Minimum bond enthalpy

Bond dissociation enthalpy

Maximum bond enthalpy

Mean bond enthalpy

-702.2 kJ

741.5 kJ

-767.8 kJ

-741.5 kJ

energy changes involved in a chemical reaction

the rate at which a reaction proceeds

the extent to which a chemical reaction proceeds

the feasibility of a chemical reaction

ΔH > 0, exothermic

ΔH < 0, exothermic

ΔH < 0, endothermic

ΔH > 0, endothermic

law of conservation of parity

law of conservation of mass

law of conservation of charge

law of conservation of energy

when one kg of it reacts with a specified amount of solvent

when one kg of it dissolves in a specified amount of solvent

when one mole of it dissolves in a specified amount of solvent

when one mole of it reacts with a specified amount of solvent

1.78 kJ.

1.09 kJ.

1.52 kJ.

1.34 kJ.

The presence of reactants in a closed vessel made up of copper is an example of a closed system.

There is an exchange of energy as well as matter between the system and the surroundings in a closed system.

The presence of reactants in a thermos flask or any other closed insulated vessel is an example of a closed system.

The presence of reacting species in a covered beaker is an example of open system

ΔH < 0, endothermic

ΔH > 0, exothermic

ΔH < 0, exothermic

ΔH > 0, endothermic

q is negative if heat is transferred to the system and w is positive if work is done on the system

q is positive if heat is transferred to the system and w is positive if work is done on the system

q is negative if heat is transferred to the system and w is negative if work is done on the system

q is positive if heat is transferred to the system and w is negative if work is done on the system

enthalpy change which occurs when one kg of an ionic compound dissociates into its ions in liquid state

enthalpy change which occurs when one mole of an ionic compound dissociates into its ions in gaseous state

enthalpy change which occurs when one mole of an ionic compound dissociates into its ions in liquid state

enthalpy change which occurs when one gm of an ionic compound dissociates into its ions in gaseous state

ΔH = −6.114 kJ mol⁻¹

ΔH = −6.415 kJ mol⁻¹

ΔH = −5.231 kJ mol⁻¹

ΔH = −7.415 kJ mol⁻¹

amount, volume, temperature

pressure, volume, temperature

pressure, volume, temperature, amount

temperature, amount, pressure

1.55 X104J

1.11 X104J

1.76 X104J

1.33 X104J