0. A 1.325 kg sample of Compound Y absorbed 5.65 kJ of heat. If the final temperature is 52.3°C, what was the initial temperature? Use your average specific heat for Compound Y. 3.78851g
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.
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**Problem:**
A 1.325 kg sample of Compound Y absorbed 5.65 kJ of heat. If the final temperature is 52.3°C, what was the initial temperature? Use your average specific heat for Compound Y.
Given calculations:
- Mass (m): 1.325 kg
- Heat absorbed (q): 5.65 kJ
- Final temperature (T₂): 52.3°C
The formula used for the calculation:
\[ q = m \cdot c \cdot \Delta T \]
Where:
- \( q \) is the heat absorbed,
- \( m \) is the mass,
- \( c \) is the specific heat,
- \( \Delta T \) is the change in temperature (\( T_2 - T_1 \)).
**Solution:**
1. Rearrange the equation to find the initial temperature (\( T_1 \)):
\[ \Delta T = \frac{q}{m \cdot c} \]
\[ T_1 = T_2 - \Delta T \]
Plug in the known values to solve.
(Note: The specific heat value for Compound Y should be known to complete the calculation.)
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