Determine the amount of heat required to raise the temperature of 0.153 kg of gold from 10.0 to 60.0 degC? ( specific heat capacity of gold= 0.128 J/g deg C) O 7.65*103 J O 490. J O 5.98*104 J O 979.2 J O 979 J
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.
![### Heat Calculation for Gold
#### Problem Statement:
Determine the amount of heat required to raise the temperature of 0.153 kg of gold from 10.0°C to 60.0°C. The specific heat capacity of gold is 0.128 J/g°C.
#### Options:
- A) \( 7.65 \times 10^3 \) J
- B) 490 J
- C) \( 5.98 \times 10^4 \) J
- D) **979.2 J** (Correct Answer)
- E) 979 J
### Explanation:
To calculate the amount of heat (Q) required, we use the formula:
\[ Q = mc\Delta T \]
where:
- \( m \) is the mass in grams (g)
- \( c \) is the specific heat capacity in J/g°C
- \( \Delta T \) is the change in temperature in °C
First, convert the mass from kg to grams:
\[ 0.153 \, \text{kg} = 153 \, \text{g} \]
Change in temperature (\( \Delta T \)):
\[ \Delta T = T_f - T_i = 60.0°C - 10.0°C = 50.0°C \]
Now, substituting the values into the formula:
\[ Q = 153 \, \text{g} \times 0.128 \, \text{J/g°C} \times 50.0°C \]
\[ Q = 979.2 \, \text{J} \]
Thus, the amount of heat required is 979.2 J.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F287ef56d-8f65-436b-964d-73a393e6640a%2Fb1ff3971-9549-427c-bf4c-1aa35af43935%2F9jm3hjl_processed.png&w=3840&q=75)
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