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

એક પ્રોટીનનું વિકૃતિકરણ (denaturation) N ⇌ D. 60°C પર, K=1 અને \(\Delta H^\circ = 666 \) kJ mol⁻¹ છે. 60°C પર \(\Delta S^\circ\) (kJ K⁻¹ mol⁻¹) સૌથી નજીક છે:

1.0 mol આદર્શ ગેસ માટે ચક્રીય પ્રક્રિયા ધ્યાનમાં લો. પ્રક્રિયા 2 અને 4 એડિયાબેટિક છે. \( R = 2 \) cal K⁻¹ mol⁻¹ વાપરો. સાચો વિકલ્પ છે:

1.0 mol आदर्श गैस के लिए चित्र में दिखाई गई ऊष्मागतिकीय प्रक्रियाओं पर विचार कीजिए। \(w_1, w_2, w_3, w_4\) क्रमशः प्रक्रिया 1, 2, 3 और 4 में किए गए कार्य को दर्शाते हैं। \(\Delta U_2\) और \(\Delta U_4\) क्रमशः प्रक्रिया 2 और 4 के लिए आंतरिक ऊर्जा में परिवर्तन हैं। \([R=2\,cal\,K^{-1}mol^{-1}]\) सही विकल्प है :

एक प्रोटीन अपनी प्रारंभिक अवस्था \(N\) से विकृत अवस्था \(D\) में \[ N \rightarrow D \] ऊष्मीय विकृतीकरण (thermal denaturation) से गुजरता है। \(60^\circ C\) पर साम्यावस्था में \(N\) और \(D\) दोनों संतुलित हैं, और विकृतीकरण का मानक एन्थैल्पी परिवर्तन \[ 666\,kJ\,mol^{-1} \] है। \(60^\circ C\) पर विकृतीकरण का मानक एंट्रॉपी परिवर्तन (\(\Delta S^\circ\)) है :

For the following reaction at 300 K: \[ \text{A}_2(g) + 3\text{B}_2(g) \rightarrow 2\text{AB}_3(g) \] The enthalpy change is \(+15 \, \text{kJ}\), then the internal energy change is:

For an endothermic reaction:
(A) \( q_p \) is negative.
(B) \( \Delta_rH \) is positive.
(C) \( \Delta_rH \) is negative.
(D) \( q_p \) is positive.
Choose the correct answer from the options given below:

Choose the correct statement for the work done in the expansion and heat absorbed or released when 5 litres of an ideal gas at 10 atmospheric pressure isothermally expands into vacuum until volume is 15 litres :

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 :

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, $\Delta H =35.5\, kJ\, mol ^{-1}$ 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)

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, △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)

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

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

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 :
\((R = 8.314\ J K^{–1} mol^{–1})\)

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 :

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-

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