Heat

First law of thermodynamics states that internal energy is a function of state and the increase in internal energy is equal to the sum of the heat supplied to the system and the work done by the system.

Mathematically:
ΔU=Q−W
Where:

ΔU = change in internal energy
Q = heat supplied to the system
W = work done by the system

1. It states that the energy of the universe remains the same.
2. Though it may be exchanged between the system and the surroundings, it can't be created or destroyed.
3. The law basically relates to the changes in energy states due to work and heat transfer.
4. It redefines the conservation of energy concept.

1. William Thomson codified the first two laws of thermodynamics.
2. He created the standard temperature scale, in which -273.15 °C was considered an absolute zero temperature, also known as OK (zero Kelvin).
3. The S.I. unit of thermodynamic temperature is Kelvin.

1. William Thomson codified the first two laws of thermodynamics.
2. He created the standard temperature scale, in which -273.15 °C was considered an absolute zero temperature, also known as OK (zero Kelvin).
3. The S.I. unit of thermodynamic temperature is Kelvin.

Celsius — temperature scale, not SI unit
Fahrenheit — temperature scale, not SI unit
Radian — unit of angle, not temperature

So, (30 × 9) / 5 = 54 degree Fahrenheit

The Kelvin scale is the absolute temperature scale used in science.0 K is called absolute zero — the lowest possible temperature, where:
Molecular motion theoretically stops
No more thermal energy can be extracted

The Kelvin scale is the absolute temperature scale used in science.
0 K is called absolute zero — the lowest possible temperature, where:
Molecular motion theoretically stops
No more thermal energy can be extracted

The SI unit of heat is expressed in joules (J).
The St unit of temperature is Kelvin (K).