This chapter covers the fundamental laws of thermodynamics, focusing on heat, work, and energy transfer in systems.
Thermodynamics – Formula & Equation Sheet
Essential formulas and equations from Physics Part - II, tailored for Class 11 in Physics.
This one-pager compiles key formulas and equations from the Thermodynamics chapter of Physics Part - II. Ideal for exam prep, quick reference, and solving time-bound numerical problems accurately.
Key concepts & formulas
Essential formulas, key terms, and important concepts for quick reference and revision.
Formulas
ΔU = Q - W
ΔU is the change in internal energy (J), Q is heat added to the system (J), and W is work done by the system (J). This is the First Law of Thermodynamics, expressing conservation of energy.
Q = m * c * ΔT
Q is heat supplied (J), m is mass (kg), c is specific heat capacity (J/kg·K), and ΔT is change in temperature (K or °C). This formula is used to calculate heat transfer when temperature changes.
PV = nRT
For an ideal gas, P is pressure (Pa), V is volume (m³), n is number of moles, R is the ideal gas constant (8.31 J/mol·K), and T is temperature (K). This is the ideal gas law.
C_p - C_v = R
C_p is molar specific heat at constant pressure, C_v is molar specific heat at constant volume, and R is the universal gas constant (8.31 J/mol·K). This relation holds for ideal gases.
W = PΔV
W is work done (J), P is pressure (Pa), and ΔV is the change in volume (m³). This formula applies when work is done by or on a gas during expansion or compression.
η = 1 - \dfrac{T_C}{T_H}
η is the efficiency of a Carnot engine, T_C is the absolute temperature of the cold reservoir (K), and T_H is the absolute temperature of the hot reservoir (K). This formula expresses the maximum efficiency of reversible heat engines.
P V^γ = constant
For a reversible adiabatic process for an ideal gas, P is pressure (Pa), V is volume (m³), and γ is the heat capacity ratio (C_p/C_v), indicating how pressure and volume relate during adiabatic changes.
Q = nC_vΔT for isochoric process
Where Q is heat added (J), n is moles of substance, C_v is molar specific heat at constant volume, and ΔT is change in temperature (K). This describes heat transfer at constant volume.
Q = nC_pΔT for isobaric process
Where Q is heat added (J), n is moles of substance, C_p is molar specific heat at constant pressure, and ΔT is change in temperature (K). This describes heat transfer at constant pressure.
S = Q/T
S is entropy (J/K), Q is heat transfer (J), and T is absolute temperature (K). This formula relates heat transfer to changes in entropy.
Equations
ΔU = Q - W
Represents the First Law of Thermodynamics indicating the relationship between internal energy change, heat added, and work done.
Q = msΔT
Formula to calculate heat supplied to or removed from a substance based on mass, specific heat, and change in temperature.
W = PΔV
Work done by the system during expansion or compression, linking pressure and volume change.
PV = nRT
Ideal gas law relating pressure, volume, and temperature for a specified amount of gas.
C_p - C_v = R
Relationship between the specific heats of an ideal gas, crucial for thermodynamic processes.
η = W_out/Q_in
Efficiency of a heat engine, representing the ratio of work output to heat input.
S = S_initial + \int{ rac{dQ}{T}}
Equation for calculating change in entropy during a thermodynamic process.
P V^γ = constant
Describes the relationship between pressure and volume during an adiabatic process.
Q = nC_pΔT for isobaric
Describes heat exchange in processes at a constant pressure.
Q = nC_vΔT for isochoric
Relates heat transfer at constant volume to change in temperature.
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