An irregular lump of an unknown metal has a measured density of 5.61 g/mL. The metal is heated to a temperature of 159 °C and placed in a graduated cylinder filled with 25.0 mL of water at 25.0 °C. After the system has reached thermal equilibrium, the volume in the cylinder is read at 31.0 mL, and the temperature is recorded as 44.6 °C. What is the specific heat of the unknown metal sample? Assume no heat is lost to the surroundings.
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.
![**Transcription for Educational Website:**
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An irregular lump of an unknown metal has a measured density of 5.61 g/mL. The metal is heated to a temperature of 159 °C and placed in a graduated cylinder filled with 25.0 mL of water at 25.0 °C. After the system has reached thermal equilibrium, the volume in the cylinder is read at 31.0 mL, and the temperature is recorded as 44.6 °C. What is the specific heat of the unknown metal sample? Assume no heat is lost to the surroundings.
\[
c = \boxed{\phantom{0000}} \quad \text{J/g} \cdot °\text{C}
\]
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**Explanation of the Diagram (if applicable):**
The provided text outlines a calorimetry experiment where an unknown metal is used to determine its specific heat. The experiment involves heating the metal and submerging it in water to observe the change in water volume and temperature once equilibrium is reached. The task is then to calculate the specific heat capacity of the metal based on given data and known formulas in calorimetry, assuming no heat loss to the surroundings.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F245e0eb4-5097-4578-8f56-633b47cf5980%2F6c8ec8f5-6d55-460c-aa66-cc7e7afb22e5%2F53x84oj_processed.jpeg&w=3840&q=75)
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