Enthalpy change for freezing of 1 g of water | vedclass

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

Question

(B) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + P\D

Vedclass · Accepted Answer

$334$

Vedclass · Answer

(B) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + P\Delta V$. At $0^{\circ} C$ and $1 \ bar$, the change in volume $(\Delta V)$ for the freezing of $1 \ g$ of water is extremely small and negligible. Therefore, $\Delta H \approx \Delta U$. Given that the enthalpy change for freezing $1 \ g$ of water is $334 \ J$, the internal energy change is also approximately $334 \ J$.

Enthalpy change for freezing of $1 \ g$ of water at $1 \ bar$ and $0^{\circ} C$ is $334 \ J$. Calculate the internal energy change in $J$ when $1 \ g$ of water is converted into ice?

Similar Questions

What is molar enthalpy of vaporization?

Expansion of a gas in vacuum is called free expansion. Calculate the work done and the change in internal energy when $1 \ L$ of ideal gas expands isothermally into vacuum until its total volume is $5 \ L$?

The relation between $\Delta H$ and $\Delta U$ is

During an isothermal expansion of an ideal gas,its:

According to thermodynamics,when can a process be called reversible?

Vedclass Test Series

Exam Paper Generator

Online Exam Module