NEET Thermodynamics Quiz
NEET-level practice on the first law, enthalpy changes and Hess's law, entropy and spontaneity - with the sign conventions written out in every solution.
Skill map
Levels in this neet thermodynamics quiz
Every question is generated fresh by AI and calibrated to your level - clear a level and the next one gets harder. Miss one and the AI tutor explains Thermodynamics until it sticks, then aims a follow-up at the gap. Want to grind one level? Start the quiz and type that sub-topic as your own.
Exam focus
How Thermodynamics is asked
A steady contributor to NEET Chemistry with a small, well-defined formula set. Questions are typically single-step numerical or direct conceptual checks on spontaneity, so it is efficient to prepare - the recurring difficulty is sign conventions rather than the physical chemistry.
Cheat sheet
Thermodynamics formulas worth memorising
| Quantity | Formula |
|---|---|
| First law | ΔU = q + w |
| Work of expansion | w = −P(ext)ΔV |
| Enthalpy and internal energy | ΔH = ΔU + Δn(g)RT |
| Hess's law | ΔH is the same by any route |
| Enthalpy from bond enthalpies | ΔH = Σ(bonds broken) − Σ(bonds formed) |
| Gibbs free energy | ΔG = ΔH − TΔS |
| Spontaneity | ΔG < 0 spontaneous, ΔG = 0 equilibrium |
Marks lost here
Common mistakes in Thermodynamics
- Getting the sign of work wrong. With ΔU = q + w, expansion by the system gives negative work. Fix one convention and apply it throughout rather than deciding case by case.
- Reversing the bond enthalpy calculation. Breaking bonds absorbs energy and forming them releases it, so ΔH is bonds broken minus bonds formed - the opposite order gives the right magnitude with the wrong sign.
- Treating spontaneous as meaning fast. ΔG describes feasibility, not rate; a reaction can be strongly spontaneous and imperceptibly slow without a catalyst.
- Assuming exothermic reactions are always spontaneous. A negative ΔH helps but does not decide it - if ΔS is negative and the temperature high enough, ΔG can still be positive.
- Forgetting to convert temperature to kelvin in ΔG = ΔH − TΔS, and to reconcile the units of ΔH (usually kJ) with ΔS (usually J per K).
Game rules
How a round works
- 01Spawn
Press play - the AI generates Thermodynamics questions in seconds.
- 02Level up
Answer to earn XP and build a streak. Difficulty adapts to your accuracy and speed.
- 03Learn or lose
Every answer - right or wrong - gets an AI tutor explanation. Wrong answers respawn as follow-ups.
Leaderboard
Thermodynamics high scores
Next challenges
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Player's guide
NEET Thermodynamics Quiz - FAQs
When is a reaction spontaneous at all temperatures?
When ΔH is negative and ΔS is positive, since ΔG = ΔH − TΔS is then negative for every temperature. If both are negative it is spontaneous only when the temperature is low; if both are positive, only when it is high.
Why is Hess's law useful?
Because enthalpy is a state function, so the total change depends only on the initial and final states and not the route. That lets you calculate the enthalpy change of a reaction that cannot be measured directly by combining reactions that can.
Is the neet thermodynamics quiz free?
Yes - completely free, with no sign-up required. Type a topic, press start, and the AI generates an adaptive Thermodynamics quiz with an explanation for every answer.
Can teachers host this neet thermodynamics quiz live for a class?
Yes - create a free teacher account, host a live room on "Thermodynamics", and students join with a 6-character code at quff.in/join. No student accounts needed.
From the blog
Thermodynamics guides & reading
NEET Thermodynamics: 30 Practice Questions with Answers
Thirty solved Thermodynamics questions at NEET level - single-step numericals and conceptual checks rather than extended calculation.
Exam PrepNEET Chemical Bonding: 30 Practice Questions with Answers
Thirty solved Bonding questions pitched at NEET's level - shapes, comparisons and trends rather than extended calculation.
More exam prep quizzes
Ready, player?
Six adaptive Thermodynamics questions. About two minutes. Climb the podium.