state and explain the first law of thermodynamics .
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Answered by
47
DEFINITION: 1ST LAW OF THERMODYNAMICS
The First Law of Thermodynamics states that energy can be converted from one form to another with the interaction of heat, work and internal energy, but it cannot be created nor destroyed, under any circumstances. Mathematically, this is represented as
ΔU=q+w
with
ΔUΔU is the total change in internal energy of a system,
qq is the heat exchanged between a system and its surroundings, and
ww is the work done by or on the system.
The First Law of Thermodynamics states that energy can be converted from one form to another with the interaction of heat, work and internal energy, but it cannot be created nor destroyed, under any circumstances. Mathematically, this is represented as
ΔU=q+w
with
ΔUΔU is the total change in internal energy of a system,
qq is the heat exchanged between a system and its surroundings, and
ww is the work done by or on the system.
Answered by
55
STATEMENT : the amount of heat supplied to a system is equal to the algebraic sum of
the change in internal energy of the system and the amount of external work done
EXPLANATION: when ∆ Q is the quantity of heat supplied to system ,a system a part of it is used to increase its internal energy ∆U and the rest is used in doing external work ∆ W .
The mathematical expression of this law is
∆Q = ∆U + ∆W .
it is a special case of the law of conservation of energy
EXAMPLE: the explosive of a fire crakers in an insulated steel drum
SIGN CONVENTION :
1) work done ∆W by the system is +ve and work done on the system is -ve
2) heat is supplied (∆Q) to the system is + ve ,heat taken from the system is -ve
3) increase in internal energy (∆U) is + ve and decrease in internal energy is -ve
the limitations of this law are
1) it does not tell about the direction of heat flow
2) it does not tell about the efficiency with which heat can be converted into work
hope it may be helpful for you
be brainly
the change in internal energy of the system and the amount of external work done
EXPLANATION: when ∆ Q is the quantity of heat supplied to system ,a system a part of it is used to increase its internal energy ∆U and the rest is used in doing external work ∆ W .
The mathematical expression of this law is
∆Q = ∆U + ∆W .
it is a special case of the law of conservation of energy
EXAMPLE: the explosive of a fire crakers in an insulated steel drum
SIGN CONVENTION :
1) work done ∆W by the system is +ve and work done on the system is -ve
2) heat is supplied (∆Q) to the system is + ve ,heat taken from the system is -ve
3) increase in internal energy (∆U) is + ve and decrease in internal energy is -ve
the limitations of this law are
1) it does not tell about the direction of heat flow
2) it does not tell about the efficiency with which heat can be converted into work
hope it may be helpful for you
be brainly
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