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1st Law of Thermodynamics

1st Law of Thermodynamics

Edited By Shivani Poonia | Updated on Jul 02, 2025 08:10 PM IST

The First Law of Thermodynamics, also known as the Law of Energy Conservation, states that energy cannot be created or destroyed but is transformable from one form to another. This is a cardinal tenet taken from classical thermodynamics and applies to every physical process. It introduces the basic concept that an independent system contains the same amount of total energy at whatever time it is considered, irrespective of the changes taking place within the system. Mathematically, this First Law is represented as ΔU=Q−W, where ΔU is the change in internal energy of the system, Q is the heat added to the system, and W is the work done by the system. This relationship emphasizes the interplay between heat, work, and internal energy.

This Story also Contains
  1. First Law or Law of Conservation of Energy
  2. Some Solved Examples
  3. Summary

First Law or Law of Conservation of Energy

It was introduced by Helmholtz and according to it "Energy can neither be created nor destroyed but can be converted from one form to another or the total energy of the universe is constant",

It can also be written as:

  • The energy of an isolated system must remain constant, although it may be transformed from one form to another.

  • Energy in one form, if it disappears will make its appearance in an exactly equivalent in another form.

  • When work is transformed into heat or heat into work, the quantity of work is mechanically equivalent to the quantity of heat.

  • It is never possible to construct a perpetual motion machine that could produce work without consuming any energy.

Thus if heat is supplied to a system it is never lost but it is partly converted into internal energy and partly in doing work in the system that is,

Heat supplied = Work done by the system + Increase in internal energy

So increase in internal energy = Heat supplied - work done by the system

ie. $\Delta E=q+w \quad[\because$ work done by the system is -w$]$

Mathematical Formulation of the First Law

If a system absorbs the 'q' amount of heat and its state changes from X to Y this heat is used up.

(i) On increasing the internal energy of the system

$\Delta \mathrm{E}=\mathrm{E}_{\mathrm{Y}}-\mathrm{E}_{\mathrm{X}}$

(ii) In order to do some external work (W) on the surroundings by the system.

From the first law, we get the relation

$
\begin{aligned}
& \Delta \mathrm{E}=\mathrm{Q}-\mathrm{W} \text { (that is, work done by the system }=\mathrm{W} \text { ) } \\
& d \mathrm{E}=d \mathrm{Q}-d \mathrm{~W} \text { or } d \mathrm{E}=d \mathrm{Q}-\mathrm{P} d \mathrm{~V})
\end{aligned}
$

Work done by the system or in expansion

OR

$
\begin{aligned}
& \Delta \mathrm{E}=\mathrm{Q}+\mathrm{W} \text { (that is, work done by the system }=\mathrm{W} \text { ) } \\
& d \mathrm{E}=d \mathrm{Q}+d \mathrm{~W} \text { or } d \mathrm{E}=d \mathrm{Q}+\mathrm{P} d \mathrm{~V})
\end{aligned}
$


Work done by the system or in compression

For the take of simplicity, remember the formula $\Delta \mathrm{E}=\mathrm{Q}+\mathrm{W}$ and when the work is done by the system, work is negative, and when the work is done on the system.

Recommended topic video on ( 1st law of Thermodynamics)

Some Solved Examples

Example 1: A heat engine absorbs heat $Q_1$ at temperature $T_1$ and heat $Q_2$ at temperature $T_1$ . Work done by the engine is $J\left(Q_1+Q_2\right)$ This data

1)violates 1st law of thermodynamics

2)violates 1st law of thermodynamics if $Q_1$ is -ve

3)violates 1st law of thermodynamics if $Q_2$ is -ve

4) (correct) does not violate 1st law of thermodynamics

Solution

As we learned in the concept:

The energy of the universe is always conserved or the total energy of an isolated system is always conserved

$\Delta E=q+W$

$\Delta E$ Internal Energy

q= Heat

w= work

This is by the 1st law of thermodynamics

Hence, the answer is the option (4).

Example 2: Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero)

1)Isochoric process: $\Delta U=q$

2) (Adiabatic process : $\Delta U=-w$

3)Isothermal process: $q=-w$

4)Cyclic process: $q=-w$

Solution

In the Adiabatic process:-

$q=0$

According to the first law of thermodynamics

$\Delta E=q+w$

So, $\Delta E=w$

Hence, the answer is the option (2).

Example 3: Which of the following will reduce the energy of the system?

1)Q=10J

2)$\Delta$V=5J

3)W=+10J

4) W=-10J

Solution

Any type of energy (Heat, Work) given to the system is positive and any type of energy taken out from the system

$W=+10 j$ i.e. 10 J work done on the system

$q=-10 j$ i.e. 10 J released by the system

W is -ve means work is being done by the system and hence its energy will decrease.

Hence, the answer is the Option (4).

Example 4: A gas undergoes change from state A to state B. In this process, the heat absorbed and work done by the gas is 5 J and 8 J, respectively. Now gas is brought back to A by another process during which 3 J of heat is evolved. In this reverse process of B to A :

Q 1)10 J of the work will be done by the gas.

2) 6 J of the work will be done by the gas.

3) 10 J of the work will be done by the surrounding on gas.

4) 6 J of the work will be done by the surrounding on gas.

Solution

Given,

A gas undergoes change from state A to state B:

$\begin{aligned} & A \longrightarrow B \\ & \mathrm{Q}=5 \mathrm{~J} \\ & \mathrm{~W}=8 \mathrm{~J} \\ & \Delta \mathrm{U}_{\mathrm{AB}}=\mathrm{Q}+\mathrm{W}=5+(-8)=-3 \mathrm{~J}\end{aligned}$

Now, gas is brought back to A from state B:

$\begin{aligned} & B \longrightarrow A \\ & \mathrm{Q}=-3 \mathrm{~J} \\ & \Delta \mathrm{U}_{\mathrm{BA}}=3 \mathrm{~J} \\ & \Delta U_{B A}=-3+W \\ & 3+3=W \\ & W=6 J\end{aligned}$

(work is done on the system)

or

As work done has a positive sign, work is done by the surrounding on the gas.

Hence, the answer is an option (4).

Example 5: A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 370 C. As it does so ,it absorbs 208 J of heat. The values of q and w for the process will be :

(R= 8.314 J/mol K) (In 7.5 = 2.01)

1)$q=+208 J, w=+208 J$

2) $q=+208 J, w=-208 J$

3)$q=-208 J, w=-208 J$

4)$q=-208 J, w=+208 J$

Solution

The process is the isothermal reversible expansion

Hence dT = 0

$\Delta$U = 0

Now, work is given by the formula

$\mathrm{W}=-\mathrm{n} \times \mathrm{R} \times \mathrm{T} \times \ln \left(\frac{\mathrm{V}_2}{\mathrm{~V}_1}\right)$

Where, R= 8.314 J/mol K, n = 0.04 moles, T = 370C = 310 K

$\mathrm{W}=-0.04 \times 8.314 \times 310 \times \ln \left(\frac{375}{50}\right)=-208 \mathrm{~J}$

Now, using 1st law of thermodynamics

$\mathrm{Q}+\mathrm{w}=\Delta \mathrm{U}$

$\therefore Q=-w=208 \mathrm{~J}$

Hence, the answer is the option (2).

Summary

The First Law of Thermodynamics, also known as the Law of Energy Conservation, states that energy cannot be created or destroyed; it can only be transformed from one form to another. In any process, the total amount of energy in an isolated system remains constant. This means that the energy you put into a system, whether as heat or work, will either increase the system's energy or be converted to another form of energy. This law is fundamental to understanding how energy works in physical and chemical processes and is crucial for fields like physics, chemistry, and engineering.

Frequently Asked Questions (FAQs)

1. What is the First Law of Thermodynamics?
The First Law of Thermodynamics states that energy cannot be created or destroyed, only converted from one form to another. In a closed system, the total energy remains constant. This law is essentially the principle of conservation of energy applied to thermodynamic systems.
2. How does the First Law of Thermodynamics relate to heat and work?
The First Law of Thermodynamics relates heat and work through the change in internal energy of a system. It states that the change in internal energy (ΔU) of a system is equal to the heat added to the system (Q) minus the work done by the system (W). This is often expressed as the equation: ΔU = Q - W.
3. Can you explain the difference between heat and internal energy?
Heat is energy transferred between systems due to a temperature difference, while internal energy is the total energy contained within a system. Heat is a process of energy transfer, whereas internal energy is a property of the system itself. When heat is added to a system, it typically increases the internal energy, but they are not the same thing.
4. Why is the First Law of Thermodynamics sometimes called the law of conservation of energy?
The First Law of Thermodynamics is often called the law of conservation of energy because it essentially states that energy cannot be created or destroyed, only converted from one form to another. This principle is fundamental to our understanding of energy conservation in all physical processes.
5. How does the First Law of Thermodynamics apply to an isolated system?
In an isolated system, there is no exchange of energy or matter with the surroundings. According to the First Law, the total energy of an isolated system must remain constant. Any changes within the system can only redistribute energy, not create or destroy it.
6. What is the significance of the term "ΔU" in the First Law equation?
ΔU represents the change in internal energy of a system. It's the difference between the final and initial internal energy states. This term is crucial because it quantifies how much the system's total energy has changed due to heat transfer and work done.
7. Can the internal energy of a system decrease? If so, how?
Yes, the internal energy of a system can decrease. This happens when the system loses more energy to its surroundings than it gains. For example, if a system does work on its surroundings or loses heat to the environment, and this energy loss is greater than any energy gained, the internal energy will decrease.
8. How does the First Law of Thermodynamics relate to endothermic and exothermic processes?
In endothermic processes, heat is absorbed by the system from the surroundings, increasing its internal energy (positive Q). In exothermic processes, heat is released from the system to the surroundings, decreasing its internal energy (negative Q). The First Law accounts for these heat transfers in calculating the overall change in internal energy.
9. What is the role of pressure-volume work in the First Law of Thermodynamics?
Pressure-volume work is one form of work considered in the First Law. It occurs when a system expands or contracts against an external pressure. The work done by the system is calculated as W = P∆V, where P is pressure and ∆V is the change in volume. This work term is included in the First Law equation: ΔU = Q - W.
10. How does the First Law of Thermodynamics apply to chemical reactions?
In chemical reactions, the First Law helps account for energy changes. The heat released or absorbed during a reaction (enthalpy change) and any work done contribute to the overall change in internal energy of the system. This law helps chemists predict and explain energy changes in reactions.
11. What is a state function, and how does it relate to the First Law?
A state function is a property that depends only on the current state of a system, not on how it reached that state. Internal energy (U) is a state function, which is why the First Law focuses on changes in U (ΔU) rather than absolute values. This means the energy change is independent of the path taken between initial and final states.
12. Can you explain the concept of adiabatic processes in relation to the First Law?
An adiabatic process is one where no heat is exchanged between the system and its surroundings (Q = 0). In this case, the First Law simplifies to ΔU = -W, meaning any change in internal energy must come solely from work done by or on the system.
13. How does the First Law of Thermodynamics apply to cyclic processes?
In a cyclic process, the system returns to its initial state after a series of changes. According to the First Law, the net change in internal energy for a complete cycle is zero (ΔU = 0). This means that the heat added to the system must equal the work done by the system over the entire cycle.
14. What is the relationship between the First Law and perpetual motion machines?
The First Law of Thermodynamics proves that perpetual motion machines of the first kind (those that produce work without energy input) are impossible. Such machines would violate the principle of energy conservation, creating energy out of nothing, which the First Law forbids.
15. How does the sign convention work in the First Law equation?
In the equation ΔU = Q - W, positive Q represents heat added to the system, while negative Q is heat removed. Positive W represents work done by the system on the surroundings, while negative W is work done on the system. This convention helps track energy flow directions.
16. What's the difference between internal energy and enthalpy?
Internal energy (U) is the total energy within a system, including kinetic and potential energy of particles. Enthalpy (H) is the sum of internal energy and the product of pressure and volume (H = U + PV). Enthalpy is often more useful for processes occurring at constant pressure, like many chemical reactions.
17. How does the First Law apply to phase changes?
During phase changes, such as melting or boiling, heat is added to or removed from a system without changing its temperature. This heat contributes to the change in internal energy by altering the potential energy between particles, as accounted for by the First Law.
18. Can you explain how the First Law relates to heat capacity?
Heat capacity is the amount of heat required to raise the temperature of a substance by one degree. The First Law relates this to internal energy: for a process at constant volume, the heat capacity (Cv) is equal to the rate of change of internal energy with temperature (∂U/∂T).
19. How does the First Law of Thermodynamics apply to living organisms?
Living organisms are open systems that exchange energy and matter with their environment. The First Law applies in that the energy input (from food) must equal the sum of energy used for work, heat production, and stored energy. This law helps explain energy balance in biological systems.
20. What is the importance of system boundaries in applying the First Law?
System boundaries are crucial in applying the First Law as they define what is included in the system and what is considered the surroundings. Proper definition of these boundaries is essential for accurately accounting for energy transfers (heat and work) between the system and its surroundings.
21. How does the First Law of Thermodynamics relate to energy efficiency?
The First Law is fundamental to understanding energy efficiency. It shows that energy can't be created, so improving efficiency means minimizing unwanted energy transfers (like heat loss) and maximizing desired energy conversions. However, it doesn't address the quality of energy, which is covered by the Second Law.
22. Can you explain how the First Law applies to gas expansion?
When a gas expands, it typically does work on its surroundings (positive W). If this expansion is adiabatic (no heat exchange), the internal energy of the gas decreases (ΔU = -W). If heat is added during expansion (like in an isothermal process), the First Law accounts for both this heat and the work done.
23. How does the First Law of Thermodynamics relate to combustion processes?
In combustion, chemical energy is converted to heat and work. The First Law accounts for this energy conversion: the change in internal energy of the system equals the heat released minus any work done. This law helps in calculating the energy output and efficiency of combustion processes.
24. What is the significance of path independence in the First Law?
Path independence means that the change in internal energy (ΔU) depends only on the initial and final states, not on the path taken between them. This is crucial because it allows us to calculate energy changes without needing to know the exact process path, simplifying many thermodynamic analyses.
25. How does the First Law apply to non-flow processes versus flow processes?
In non-flow processes, the system's mass remains constant, and the First Law is applied as ΔU = Q - W. In flow processes, where mass enters or leaves the system, the law is modified to include the energy associated with this mass flow, often expressed using enthalpy instead of internal energy.
26. Can you explain the concept of internal energy in ideal gases using the First Law?
For an ideal gas, the internal energy depends only on temperature, not on pressure or volume. The First Law helps us understand that in processes where an ideal gas's temperature doesn't change (like isothermal expansion), the internal energy remains constant, and any heat added must equal the work done.
27. How does the First Law of Thermodynamics relate to energy storage technologies?
The First Law is crucial in energy storage technologies. It dictates that energy stored must equal energy input minus losses. This law guides the design of storage systems to minimize energy losses and maximize the amount of useful energy that can be retrieved from the storage process.
28. What is the relationship between the First Law and thermochemistry?
Thermochemistry heavily relies on the First Law. It uses this law to track energy changes in chemical reactions, often focusing on heat transfers at constant pressure (enthalpy changes). The law helps in calculating reaction energies, bond energies, and predicting the heat released or absorbed in chemical processes.
29. How does the First Law apply to reversible versus irreversible processes?
The First Law applies equally to both reversible and irreversible processes, as it only concerns the conservation of energy. However, reversible processes are idealized scenarios where the system is always in equilibrium, while irreversible processes involve non-equilibrium states. The energy accounting using the First Law remains valid for both.
30. Can you explain how the First Law relates to the concept of work in thermodynamics?
The First Law incorporates work as a means of energy transfer between a system and its surroundings. Work in thermodynamics is defined as force acting through a distance, often manifesting as pressure-volume work in gases. The law shows that work done by or on a system directly affects its internal energy.
31. How does the First Law of Thermodynamics apply to heat engines?
In heat engines, the First Law helps account for energy conversions. It shows that the work output of an engine (W) is equal to the difference between the heat input from a hot reservoir (Qh) and the heat rejected to a cold reservoir (Qc): W = Qh - Qc. This law sets the foundation for understanding engine efficiency.
32. What is the significance of constant volume processes in relation to the First Law?
In constant volume processes, no pressure-volume work is done (W = 0). The First Law then simplifies to ΔU = Q, meaning all heat added to the system goes directly into changing its internal energy. This is particularly useful in analyzing reactions in sealed containers or in determining heat capacities at constant volume.
33. How does the First Law help in understanding the energy changes in phase transitions?
During phase transitions, like melting or vaporization, heat is added to a system without changing its temperature. The First Law accounts for this energy input as an increase in internal energy, specifically as an increase in the potential energy between particles as they change from one phase to another.
34. Can you explain how the First Law applies to isothermal processes?
In isothermal processes, temperature remains constant. For an ideal gas, this means the internal energy doesn't change (ΔU = 0). The First Law then shows that any heat added to the system must be equal to the work done by the system (Q = W). This is crucial in understanding processes like isothermal expansion or compression.
35. How does the First Law of Thermodynamics relate to calorimetry experiments?
Calorimetry relies heavily on the First Law. In these experiments, the heat exchanged in a process is measured by observing temperature changes in a known quantity of a substance (usually water). The First Law allows us to equate this heat exchange to changes in internal energy or enthalpy of the system being studied.
36. What is the importance of understanding system types (open, closed, isolated) when applying the First Law?
Understanding system types is crucial for correctly applying the First Law. In closed systems, energy can be exchanged but not matter. In open systems, both energy and matter can be exchanged. In isolated systems, neither energy nor matter is exchanged. The First Law is applied differently in each case, accounting for the relevant energy and mass transfers.
37. How does the First Law help in analyzing chemical bond formation and breaking?
The First Law helps in analyzing bond energies by accounting for the energy changes when bonds are formed or broken. Bond formation typically releases energy (exothermic), while bond breaking requires energy input (endothermic). The overall energy change in a reaction, as dictated by the First Law, is the net result of all bond breaking and forming processes.
38. Can you explain how the First Law applies to non-ideal gases?
For non-ideal gases, internal energy depends on both temperature and volume, unlike ideal gases. The First Law still applies, but calculations become more complex. It accounts for intermolecular forces and volume effects on internal energy, requiring more sophisticated equations of state to accurately describe energy changes.
39. How does the First Law of Thermodynamics relate to the concept of enthalpy of formation?
The enthalpy of formation is the heat change when one mole of a compound is formed from its elements in their standard states. The First Law allows us to calculate these values by measuring heat changes in reactions. These enthalpies are crucial for predicting overall energy changes in more complex chemical reactions.
40. What is the significance of the First Law in understanding energy diagrams for chemical reactions?
Energy diagrams for reactions are based on the First Law. They show how the internal energy or enthalpy of a system changes during a reaction. The law helps in interpreting these diagrams, showing energy barriers (activation energy) and overall energy changes (ΔH or ΔU) for the reaction, which are crucial for understanding reaction kinetics and thermodynamics.
41. How does the First Law apply to systems undergoing multiple simultaneous processes?
When a system undergoes multiple processes simultaneously, the First Law allows us to sum up all energy contributions. The total change in internal energy is equal to the net heat added minus the net work done, considering all processes. This principle is crucial in analyzing complex systems like chemical plants or living organisms.
42. Can you explain how the First Law relates to the concept of state functions in thermodynamics?
The First Law introduces the concept of state functions in thermodynamics. Internal energy (U) is a state function, meaning its change depends only on the initial and final states, not the path taken. This property of U, as defined by the First Law, extends to other thermodynamic quantities like enthalpy, entropy, and Gibbs free energy.
43. How does the First Law of Thermodynamics apply to electrochemical cells?
In electrochemical cells, the First Law helps account for the conversion of chemical energy to electrical energy. The change in internal energy of the system is related to the heat produced and the electrical work done. This law is crucial in understanding the energy efficiency and maximum work output of batteries and fuel cells.
44. What is the role of the First Law in understanding heat pump operations?
Heat pumps move heat from a cold reservoir to a hot reservoir, requiring work input. The First Law helps quantify the energy transfers involved: the work input plus the heat extracted from the cold reservoir equals the heat delivered to the hot reservoir. This law is essential for calculating the efficiency and performance of heat pumps.
45. How does the First Law help in analyzing the energy changes in solution processes?
The First Law is crucial in understanding solution processes. It accounts for the energy changes when solutes dissolve in solvents, including heat absorbed or released (solution enthalpy). This law helps explain why some dissolution processes are endothermic while others are exothermic, based on the net energy change of breaking and forming interactions.
46. Can you explain how the First Law applies to adiabatic compression and expansion?
In adiabatic processes, no heat is exchanged with the surroundings (Q = 0). The First Law then states that the change in internal energy is solely due to work done: ΔU = -W. For compression, work is done on the system, increasing its internal energy and temperature. For expansion, the system does work, decreasing its internal energy and temperature.
47. How does the First Law of Thermodynamics relate to the concept of bond dissociation energy?
Bond dissociation energy is the energy required to break a particular chemical bond. The First Law helps

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