Thermal Physics Q&A: Get Expert Help and Learn from Real-World Examples

What thermodynamic properties are extensive?

The normal boiling point of water is 100 Celcius and the molar enthalpy of vaporization of water is 40.7 KJ/mol. What is the boiling point of water under a pressure of 0.500 atm?

What is the difference b/n spontaneity criterial of simple and non simple systems in terms of gibbs and helmholtz free energies?

The change in temperature and pressure required to bring a sample of water at ${25}^{\circ <!--\; \circ \; -->}C$ and 1 atm of pressure to it triple point.

What is Helmholtz free energy ?

While heating two different samples of water at sea level one boils at 102°C and one boils at 99.2°C calculate the percentage error for each sample from the theoretical hundred degrees Celsius

At what conditions of a system can the equation of Helmholtz free energy be applied? Select one:a. T- const V- const
b. T= const U = const
c. V- const M -const
d. M = const P- const

Let the system be one mole of argon gas at room temperature and atmospheric pressure. Compute the total energy (kinetic only, neglecting atomic rest energies), entropy, enthalpy, Helmholtz free energy, and Gibbs free energy. Express all answers in SI units.

At high altitudes, the ambient air pressure can be significantly less than 1 bar, so water boils at a lower temperature than 100 C. What is the boiling point of water at an altitude where the ambient air pressure is 0.72 bar? The enthalpy of vaporization of water near its boiling point is 40.7 kJ/mol.

What calorimetry approach is this?
Question:
Find the final tempertature of the system when $5gm$ of steam at ${100}^{\circ <!--\; \circ \; -->}C$ is mized with $31.5gm$ ice at $-<!--\; -\; -->{20}^{\circ <!--\; \circ \; -->}C$
Constants:
Specific heat of ice and specific heat of steam is $0.5cal/gm{/}^{\circ <!--\; \circ \; -->}C$
Specific heat of water is $1cal/gm{/}^{\circ <!--\; \circ \; -->}C$
Latent heat of fusion is $80cal/gm$
Latent heat of vaporization is $540cal/gm$
My attempt:
I usually approach these problems by setting the final temperature as $T$. Then, I equate heat lost by steam to heat gained by ice. I have been taught this method and I am adept at it.
My problem: The solution given in my workbook is:
Heat released when $1g$ of steam at ${100}^{\circ <!--\; \circ \; -->}C$ is cooled to $-<!--\; -\; -->{20}^{\circ <!--\; \circ \; -->}C$ is $730cal$. Now, this heat is given to be given to $1+6.3g=7.3g$ of ice. This raises the temperature by ${10}^{\circ <!--\; \circ \; -->}C$
This is a new method for me, and I am unable to understand it. I wish to know:
How does this method work? In what calorimetry situations can this method be applied?
NOTE: The final answer is ${10}^{\circ <!--\; \circ \; -->}C$

The boiling point of an aqueous solution containing a nonvolatile electrolyte is ${100.75}^{\circ <!--\; \circ \; -->}C$
What is the boiling point elevation?

What molality of a nonvolatile, nonelectrolyte solute is needed to raise the boiling point of water by ${7.10}^{\circ <!--\; \circ \; -->}C(K_b={0.520}^{\circ <!--\; \circ \; -->}C/m)$ ?

Calculate delta G and delta A for the freezing of 1.00 mol of H2O at 0oC and 1 atm. The heat of fusion of water at 0oC is 6002 J mol-1. The density of ice at 0oC and 1 atm is 0.917 g cm-3, and that of water at the same conditions is 1.000 g cm-3.
The correct answers are 0; -0.16 respectively but i'm getting a different one