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Online Practice: The first law of thermodynamics: Concept of work, heat, internal energy and enthalpy, heat capacity, molar heat capacity for JEE

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Sharpen your chemistry preparation with interactive online practice for The first law of thermodynamics: Concept of work, heat, internal energy and enthalpy, heat capacity, molar heat capacity. Goodmarks offers 37+ JEE-style MCQs mapped to the official syllabus, each with detailed explanations so you learn from every attempt.

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Part of Chemical Thermodynamics in JEE Main Chemistry.

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Q1ChemistryUnit 4: Chemical Thermodynamics

Which of the following statement(s) is/are true? "Internal energy of an ideal gas

Q2ChemistryUnit 4: Chemical Thermodynamics

When 229 J of energy is supplied as heat at constant pressure to 3 mol

A r(g),

the temperature of the sample is increased by

2.55 \mathrm{K}

. Calculate the motor heat capacity at constant volume:

Q3ChemistryUnit 4: Chemical Thermodynamics

An ideal gas is compressed in a closed container its U?

Q4ChemistryUnit 4: Chemical Thermodynamics

Root mean square velocity of molecules of a diatomic gas is to be increased to 1.5 times, If the process is done adiabtically, the ratio of initial volume to the final volumes is :

Q5ChemistryUnit 4: Chemical Thermodynamics

Under which of the following conditions is the relation,

\triangle \boldsymbol{H}=\triangle \boldsymbol{U}+\boldsymbol{P} \triangle \boldsymbol{V}

valid for a closed system?

Q6ChemistryUnit 4: Chemical Thermodynamics

The molar enthalpy change for

\boldsymbol{H}_{2} \boldsymbol{O}(l) \rightleftharpoons \boldsymbol{H}_{2} \boldsymbol{O}(\boldsymbol{g})

\boldsymbol{3} \boldsymbol{7} \boldsymbol{3} K

and

\boldsymbol{1}

\boldsymbol{m}

41 k J /

mol. Assuming ideal behavior the internal energy change for vaporization of 1 mol of water at

373 K

and 1 atm in

\mathrm{kJ} \mathrm{mol}^{-1}

is:

Q7ChemistryUnit 4: Chemical Thermodynamics

Calculate the temperature of a hydrogen-oxygen flame assuming that the gases at

25^{\circ} \mathrm{C}

are mixed in stoichiometric proportion and react completely to give

H_{2} O(g) . \Delta H_{298}^{\circ}

of combustion of

\boldsymbol{H}_{2}

-\mathbf{5 8}

kcal

\boldsymbol{m o l}^{-1}

The reaction is at constant pressure and the

C_{p}

values are

(7 / 2) R

for each gas.

(\boldsymbol{R}=\mathbf{2} \boldsymbol{c} \boldsymbol{a} \boldsymbol{l})

Q8ChemistryUnit 4: Chemical Thermodynamics

Assertion

C_{P}-C_{V}=R

for an ideal gas. Reason

\left[\frac{\partial E}{\partial V}\right]_{T}=0

for an ideal gas.

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