(C) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta E)$ is given by the equation: $\Delta H = \Delta E + \De

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(C) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta E)$ is given by the equation: $\Delta H = \Delta E + \Delta n_g RT$. For the reaction $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$,the change in the number of moles of gaseous species is calculated as: $\Delta n_g = n_{p(g)} - n_{r(g)} = 1 - (1 + 0.5) = 1 - 1.5 = -0.5$. Since $\Delta n_g = -0.5$ (which is negative),the term $\Delta n_g RT$ is negative. Therefore,$\Delta H = \Delta E - 0.5 RT$,which implies that $\Delta H < \Delta E$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

At constant $T$ and $P$,which one of the following statements is correct for the reaction,$CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$?

AIIMS 1982 All AIIMS

AIIMS 1983 All AIIMS

A
$\Delta H$ is independent of the physical state of the reactants of that compound
B
$\Delta H > \Delta E$
C
$\Delta H < \Delta E$
D
$\Delta H = \Delta E$

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

Thermodynamics

Subtopic

First law of thermodynamics

Previous Year

AIIMS 1982 Paper All AIIMS years →

Previous Year

AIIMS 1983 Paper All AIIMS years →

$A$ gas absorbs $120 \text{ J}$ of heat and expands by $300 \times 10^{-6} \text{ m}^3$ against a constant external pressure of $2 \times 10^5 \text{ Nm}^{-2}$. What will be the change in internal energy of the system (in $\text{ J}$)?

DifficultMHT CET 2026

View Solution

If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas,then

EasyKCET 2008

View Solution

Standard enthalpy of vaporisation $\Delta_{vap}H^o$ for water at $100\ ^oC$ is $40.66\ kJ\ mol^{-1}.$ The internal energy of vaporisation of water at $100\ ^oC$ (in $kJ\ mol^{-1}$) is ............... $kJ\ mol^{-1}$ (Assume water vapour to behave like an ideal gas)

EasyAIPMT 2012

View Solution

At a certain temperature, $T(K)$, during a process, $500 \text{ J}$ is absorbed by the system and work of $200 \text{ J}$ is done by the system. Then the change in internal energy of the system is: (in $\text{ J}$)

MediumNEET 2026

View Solution

For the reaction $FeCO_{3(s)} \to FeO_{(s)} + CO_{2(g)}$,$\Delta H = 82.8 \ kJ$ at $25 \ ^oC$. What is $\Delta U$ at $25 \ ^oC$ in $kJ$?

Medium

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

At constant $T$ and $P$,which one of the following statements is correct for the reaction,$CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$?

Similar Questions

$A$ gas absorbs $120 \text{ J}$ of heat and expands by $300 \times 10^{-6} \text{ m}^3$ against a constant external pressure of $2 \times 10^5 \text{ Nm}^{-2}$. What will be the change in internal energy of the system (in $\text{ J}$)?

If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas,then

Standard enthalpy of vaporisation $\Delta_{vap}H^o$ for water at $100\ ^oC$ is $40.66\ kJ\ mol^{-1}.$ The internal energy of vaporisation of water at $100\ ^oC$ (in $kJ\ mol^{-1}$) is ............... $kJ\ mol^{-1}$ (Assume water vapour to behave like an ideal gas)

At a certain temperature, $T(K)$, during a process, $500 \text{ J}$ is absorbed by the system and work of $200 \text{ J}$ is done by the system. Then the change in internal energy of the system is: (in $\text{ J}$)

For the reaction $FeCO_{3(s)} \to FeO_{(s)} + CO_{2(g)}$,$\Delta H = 82.8 \ kJ$ at $25 \ ^oC$. What is $\Delta U$ at $25 \ ^oC$ in $kJ$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module