Significance of First Law Of Thermodynamic

The first law of thermodynamics states that "Energy cannot be both created and destroyed, according to this. in other words, a system's energy is constant. Thus, the amount of energy in the system is constant both before and after the process (as in chemistry). It can, however, be transferred from one location to another and converted to and from other forms of energy.".
"We" are the most simple example of 1st law of thermodynamics
Energy we intake in form of food is stored in our body and part of it is lost in our activities or dissipated as body heat. This means that before and after the process ( as in chemistry), the amount of energy in the system remains the same.
OTHER EXAMPLES ARE: 
Electric bulb which transfers electrical energy into light energy, when we walk or run chemical energy stored in body is transform into kinetic energy, Our universe is an isolated system so the change in energy of our universe is always zero, ...consider a hot coffee on the table after some time we see that the coffee becomes cold(relatively) this is due to the heat dissipation from the coffee to the room...

SIGNIFICANCE
These are the following significance of 'First Law of Thermodynamics':
(1) The first significance is related with law of conservation of energy, heat and work both are different forms of same entity known as energy which is conserved
(2) Energy of isolated system is constant. Example: Universe
(3) You cannot have a device which gives output as work without any heat input.This device is known as perpetual motion machine of 1st kind which is not possible.

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