Answer:Heat and work are two different ways of transferring energy from one system to another. The the distinction between Heat and Work is important in the field of thermodynamics. Heat is the transfer of thermal energy between systems, while work is the transfer of mechanical energy between two systems.
The main relationship is the change in energy of a closed system is equal to the heat added to the system plus work done on the system. This total energy is usually represented by U, so Delta U = Q + W. For flow systems we define enthalpy as H the change of which is also equal to Q + W. There are a number of restrictions on this formula, mainly if there are other forms of energy besides work involved, such as changes in potential energy or electromagnetic field energy etc. This is the first law of thermodynamics.
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Answer:Heat and work are two different ways of transferring energy from one system to another. The the distinction between Heat and Work is important in the field of thermodynamics. Heat is the transfer of thermal energy between systems, while work is the transfer of mechanical energy between two systems.
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Answer:
The main relationship is the change in energy of a closed system is equal to the heat added to the system plus work done on the system. This total energy is usually represented by U, so Delta U = Q + W. For flow systems we define enthalpy as H the change of which is also equal to Q + W. There are a number of restrictions on this formula, mainly if there are other forms of energy besides work involved, such as changes in potential energy or electromagnetic field energy etc. This is the first law of thermodynamics.
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