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

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Short tricks for The first law of thermodynamics: Concept of work, heat, internal energy and enthalpy, heat capacity, molar heat capacity work only with strong fundamentals. Apply the tips below in timed sets and review every explanation.

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  • The first law of thermodynamics: Concept of work, heat, internal energy and enthalpy, heat capacity, molar heat capacity focus drill

    Solve 15 mixed MCQs for The first law of thermodynamics: Concept of work, heat, internal energy and enthalpy, heat capacity, molar heat capacity, review every explanation, and note formulas you hesitated on.

  • NCERT line recall

    For Inorganic, exact NCERT phrasing often matches the correct option — highlight one-liners during revision.

  • Balance then compare

    In Physical Chemistry numericals, write the balanced relation first, then substitute values with units.

Syllabus context

Part of Chemical Thermodynamics in JEE Main Chemistry.

Free sample questions

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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 Ar(g),A r(g), the temperature of the sample is increased by 2.55K2.55 \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, △H=△U+P△V\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 H2O(l)⇌H2O(g)\boldsymbol{H}_{2} \boldsymbol{O}(l) \rightleftharpoons \boldsymbol{H}_{2} \boldsymbol{O}(\boldsymbol{g}) at 373K\boldsymbol{3} \boldsymbol{7} \boldsymbol{3} K and 1\boldsymbol{1} at m\boldsymbol{m} is 41kJ/41 k J / mol. Assuming ideal behavior the internal energy change for vaporization of 1 mol of water at 373K373 K and 1 atm in kJmol−1\mathrm{kJ} \mathrm{mol}^{-1} is:
Q7ChemistryUnit 4: Chemical Thermodynamics
Calculate the temperature of a hydrogen-oxygen flame assuming that the gases at 25∘C25^{\circ} \mathrm{C} are mixed in stoichiometric proportion and react completely to give H2O(g).ΔH298∘H_{2} O(g) . \Delta H_{298}^{\circ} of combustion of H2\boldsymbol{H}_{2} is −58-\mathbf{5 8} kcal mol−1\boldsymbol{m o l}^{-1} The reaction is at constant pressure and the CpC_{p} values are (7/2)R(7 / 2) R for each gas. (R=2cal)(\boldsymbol{R}=\mathbf{2} \boldsymbol{c} \boldsymbol{a} \boldsymbol{l})
Q8ChemistryUnit 4: Chemical Thermodynamics
Assertion CP−CV=RC_{P}-C_{V}=R for an ideal gas. Reason [∂E∂V]T=0\left[\frac{\partial E}{\partial V}\right]_{T}=0 for an ideal gas.

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