Respuesta :
The change in the internal energy of the system is [tex]\boxed{ - 1{\text{278200 J}}}[/tex].
Further explanation:
Thermodynamics:
The branch of chemistry that deals with heat, temperature and its connection with work is known as thermodynamics. It has wide uses in pyrometallurgy, gas-phase reaction gas-solid reaction, and ATP generation.
First law of Thermodynamics:
It is based on the law of energy conservation that states total energy of system to be constant. According to this law, internal energy change is determined by sum of work done on the system and heat supplied. Its mathematical expression is as follows:
[tex]\Delta {\text{U}} = {\text{q}} - {\text{W}}[/tex] …… (1)
Here,
[tex]\Delta {\text{U}}[/tex] is the change in internal energy of the system.
q is the heat released by the system.
W is the work done to the system.
The value of W is 425 kcal.
The value of q is [tex]5 \times {10^2}{\text{ kJ}}[/tex].
Substitute these values in equation (1).
[tex]\begin{aligned}\Delta {\text{U}} &= \left( {5 \times {{10}^2}{\text{ kJ}}}\right)\left( {\frac{{{{10}^3}{\text{ J}}}}{{1{\text{ kJ}}}}} \right)-\left( {425{\text{ kcal}}}\right)\left( {\frac{{{{10}^3}{\text{ cal}}}}{{1{\text{ kcal}}}}} \right)\left( {\frac{{4.184{\text{ J}}}}{{1{\text{ cal}}}}} \right)\\& =500000{\text{ J}} - 1778200{\text{ J}}\\&=- 1{\text{278200 J}}\\\end{aligned}[/tex]
Therefore the change in internal energy of the system is -1278200 J.
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Thermodynamics
Keywords: internal energy, heat, work, q, W, P, -1278200 J, thermodynamics, first law of thermodynamics, law of conservation of energy, total energy, isolated system, change in internal energy.
Work done is defined as the energy transferred by the system to its surrounding. The internal energy of the system is -1278200 J.
Law of energy conservation states that the total energy of an isolated system is constant. The internal energy change is determined by the sum of work done and heat supplied. The equation can be written as:
- [tex]\Delta \text {U&= q - W}[/tex]
where,
- [tex]\Delta \text U[/tex] = change in internal energy
- q = heat released by the system.
- W = work done to the system.
Given that,
- W = 425 kcal
- q = 5 [tex]\times 10^2[/tex]
Now, substituting the values in above equation:
[tex]\begin{aligned}\Delta \text{U} &= (5 \times 10 ^2)\times \dfrac{10^3\text{J}}{1 \text{kJ}} \;-\;(425 \text{kcal})\;\times\;\dfrac{10^3\text{J}}{1 \text{kJ}} \times\dfrac{4.184\text{J}}{1 \text{cal}} \\\\&= 500000 \;\text J\;-\;1778200 \;\text J\\\\&= -1278200\;\text J\end {aligned}[/tex]
Therefore, the change in internal energy of the system is -1278200 J.
To know more about internal energy, refer to the following link:
https://brainly.com/question/14035409?referrer=searchResults
