Assertion : The increase in internal energy ( | vedclass

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

Question

(D) The vaporization of water is a phase change process occurring at constant temperature $(373 \ K)$.For an ideal gas,internal energy $(E)$ is a func

Vedclass · Accepted Answer

If both the Assertion and Reason are incorrect.

Vedclass · Answer

(D) The vaporization of water is a phase change process occurring at constant temperature $(373 \ K)$.For an ideal gas,internal energy $(E)$ is a function of temperature only,so $\Delta E = 0$ for isothermal processes.However,for real substances like water undergoing a phase change,the internal energy changes because the intermolecular forces are overcome during vaporization.Therefore,the Assertion is incorrect because $\Delta E 
eq 0$ for the vaporization of water.The Reason is also incorrect because $\Delta E = 0$ only strictly applies to ideal gases in isothermal processes,and even then,it does not account for phase changes where potential energy changes.

Assertion : The increase in internal energy $(\Delta E)$ for the vaporization of one mole of water at $1 \ atm$ and $373 \ K$ is zero.
Reason : For all isothermal processes,$\Delta E = 0$.

Similar Questions

$C_{(s)} + 2 H_{2(g)} \rightarrow CH_{4(g)}$; $\Delta H = -74.8 \ kJ \ mol^{-1}$
Which of the following diagrams gives an accurate representation of the above reaction?
[$R \rightarrow$ reactants; $P \rightarrow$ products]

For the reaction $2A_{(g)} + B_{(g)} \to 2D_{(g)}$,given $\Delta U^{\theta} = -10.5 \ kJ$ and $\Delta S^{\theta} = -44.1 \ J \ K^{-1}$. Calculate $\Delta G^{\theta}$ for the reaction at $298 \ K$ and predict whether the reaction may occur spontaneously.

Which of the following relations are correct?
$(A)$ $\Delta U = q + p \Delta V$
$(B)$ $\Delta G = \Delta H - T \Delta S$
$(C)$ $\Delta S = \frac{q_{rev}}{T}$
$(D)$ $\Delta H = \Delta U - \Delta nRT$
Choose the most appropriate answer from the options given below:

The amount of heat released when $20 \ mL$ of $0.5 \ M$ $NaOH$ is mixed with $100 \ mL$ of $0.1 \ M$ $HCl$ is $x \ kJ$. The heat of neutralization is:

Which graph represents an exothermic reaction?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Assertion : The increase in internal energy $(\Delta E)$ for the vaporization of one mole of water at $1 \ atm$ and $373 \ K$ is zero.Reason : For all isothermal processes,$\Delta E = 0$.