The following information is given for cadmium at 1 atm: Boiling point 765.0°C Heat of vaporization = 213 cal/g Melting point = 321.0°C Heat of fusion 13.0 cal/g = 9 for this question. Heat is added to a sample of solid cadmium at its normal melting point of 321.0°C. How many grams of cadmium will melt if 1.69 kcal of energy are added?
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![**Educational Content: Cadmium Phase Change Calculation**
**Given Information:**
For cadmium at 1 atm:
- **Boiling point:** 765.0°C
- **Heat of vaporization:** 213 cal/g
- **Melting point:** 321.0°C
- **Heat of fusion:** 13.0 cal/g
**Problem:**
Calculate the grams of cadmium that will melt at its normal melting point of 321.0°C when 1.69 kcal of energy is added.
**Procedure:**
To find the amount of cadmium that melts, use the heat of fusion formula:
\[
\text{Heat required for fusion} = \text{mass} \times \text{heat of fusion}
\]
Here, the energy provided is 1.69 kcal, which is equal to 1690 cal (since \(1 \text{kcal} = 1000 \text{cal}\)).
Given:
- Heat of fusion for cadmium = 13.0 cal/g
- Total energy provided = 1690 cal
**Calculation:**
\[
\text{mass} = \frac{\text{Total energy}}{\text{Heat of fusion}} = \frac{1690 \text{ cal}}{13.0 \text{ cal/g}}
\]
\[
\text{mass} = 130 \text{ g}
\]
Therefore, 130 grams of cadmium will melt when 1.69 kcal of energy is added.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc23f13d4-22d2-4ccd-93de-be9deaee328b%2F219acada-78a3-4665-be01-c1707c711c45%2Ftpmmfd_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
