List of top Chemistry Questions on Thermodynamics asked in NEET (UG)

The right option for the mass of CO₂ produced by heating 20g of 20% pure limestone is 
(Atomic mass of Ca= 40) 

Which amongst the following options is the correct relation between change in enthalpy and change in internal energy

Which of the following p-V curve represents maximum work done?

The maximum temperature that can be achieved in blast furnace is :

Under isothermal condition, a gas at 300 K expands from 0.1 L to 0.25 L against a constant externalpressureof2bar Theworkdonebythe gas i s : [Given that 1Lbar= 100J)

In which case change in entropy is negative ?

A gas is allowed to expand in a well insulated container against a constant external pressure of $2.5\, atm$ from an initial volume of $2.50\, L$ to a final volume of $4.50\, L$. The change in internal energy $\Delta U$ of the gas in joules will be

For a given reaction, △H = 35.5 kJ mol^–1 and △S = 83.6 JK–1 mol^–1. The reaction is spontaneous at  :
(Assume that△H and △S do not vary with temperature)

A gas is allowed to expand in a well insulated container against a constant external pressure of 2.5 atm from an initial volume of 2.50 L to a final volume of 4.50 L. The change in internal energy △U of the gas in joules will be

For a given reaction, $\Delta H =35.5\, kJ\, mol ^{-1}$ and $\Delta S =83.6\, JK ^{-1}\, mol ^{-1} .$ The reaction is spontaneous at $:$ (Assume that $\Delta H$ and $\Delta S$ do not vary with temperature)

Consider the following liquid-vapour equilibrium ${Liquid <=> Vapour }$ Which of the following relations is correct ?

For a sample of perfect gas when its pressure is changed isothermally from $p_i$ to $p_f$, the entropy change is given by

For the reaction:
\(X_2O4(l) → 2XO_2(g)\)
△U = 2.1 k cal, △S = 20 cal K^–l at 300 K.
Hence △G is

Using the Gibbs energy change, \(△G° = + 63.3\  kJ\), for the following reaction,
\(Ag_2CO_3 (g) ⇋ 2Ag+ (aq) + CO_3^{2–} (aq)\)
the \(K_{sp}\) of \(Ag_2CO_3 \)(s) in water at \(25°C\) is :
\((R = 8.314\ J K^{–1} mol^{–1})\)

Which of the following statements is correct for the spontaneous adsorption of a gas?

A reaction having equal energies of activation for forward and reverse reactions has :-

The enthalpy of fusion of water is $1.435\, kcal/mol.$ The molar entropy change for the melting of ice at $0^{\circ}C$ is :

Enthalpy change for the reaction, $4 H _{( g )} \rightarrow 2 H _{2( g )}$ is $-869.6\, kJ$ The dissociation energy of $H - H$ bond is

Consider the following processes : $\Delta H (kJ / mol)$ ½ A → B + 150 3B → 2C + D -125 E + A → 2D +350 For B + D → E + 2C, ΔH will be-

Which of the following is correct option for free expansion of an ideal gas under adiabatic condition ?

Three moles of an ideal gas expanded spontaneously into vaccum. The work done will be

The following two reactions are known ${Fe2O3(s) + 3CO(g) -> 2Fe(s) + 3CO2(g); \Delta H = - 26.8 \, kJ }$ ${FeO(s) + CO (g) -> Fe(s) + CO2(g); \Delta H - 16.5 \, kJ}$ The value of $\Delta H$ for the following reaction ${Fe2O3(s) + CO(g) -> 2FeO(s) + CO2(g) }$ is

For vaporization of water at 1 atmospheric pressure, the values of $\Delta H$ and $\Delta S$ are $40.63 \, kJ \, mol^{-1}$ and $108.8 \, JK^{-1} mol^{-1}$, respectively. The temperature when Gibbs energy change $(\Delta G)$ for this transformation will be zero, is

From the following bond energies : $H - H$ bond energy $: 431.37\, kJ\, mol ^{-1}$ $C = C$ bond energy $: 606.10\, kJ\, mol ^{-1}$ $C - C$ bond energy $: 336.49\, kJ\, mol ^{-1}$ $C - H$ bond energy $: 410.50\, kJ\, mol ^{-1}$ Enthalpy for the reaction, will be

Which of the following are not state functions? (I) q + W (II) q (III) w (IV) H-TS