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Is in the adiabatic process change in internal energy is equal to change in work done?
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Why does temperature of gas drops in an adiabatic process?
because in adiabatic process heat absorbed is zero. and the work is done by internal energy. so internal energy decreases.we know that temperature is directly related with internal energy
In Adiabatic process how the ideal gases increases it's internal energy?
The first law of thermodynamics states that: DU = DQ + DW where DU is the increase in the internal energy of the gas DQ is the heat supplied to the system and DW is the work done ON the system For an adiabatic process, DQ = 0 Therefore, DU = DW It can be thus easily seen that for the internal to increase (DU +ve), DW must be positive, that is work has to be done on the system (in this case the ideal gas). Hence, the gas should be compressed.
How is heat provided in adiabatic process?
First we measured the temperature of the sample and then give certain amount of heat to it. Then we will measure the final temperature and divide amount of heat supplied to increase in temperature, gives the heat capacity of the sample.
When 430 J of work is done on a system it lost 120 J energy as heat Calculate the value of internal energy change for this process?
The first law of thermodynamics requires that energy input must equal energy output plus energy accumulation. In this case that translates to; 430 J = 120 J + (internal energy change) so Internal energy change = 430 J - 120 J = +310 J (the internal energy increased by 310 Joules)
Which thermodynamic process takes place at a constant temperature so that the internal energy of a system remains unchanged?
If a thermodynamic process takes place at a constant temperature it is called "isothermal". A word of caution however: the internal energy of a system may not remain the same in an isothermal process if the composition or phase changes; e.g. melting ice can be an isodthermal process but there is certainly a change in internal energy when it happens.
Why does temperature of gas drops in an adiabatic process?
because in adiabatic process heat absorbed is zero. and the work is done by internal energy. so internal energy decreases.we know that temperature is directly related with internal energy
How does the temperature of gas change when it is compressed if the process is adiabatic?
In an adiabatic process, the temperature is increased when it is compressed. There is an increase in internal kinetic energy, and because temperature is related to kinetic energy, it is also increased.
Why do adiabatic temperature changes occur?
In adiabatic process heat is neither added nor removed from the system. So the work done by the system (expansion) in adiabatic process will result in decrease of internal energy of that system (From I st law). As internal energy is directly proportional to the change in temperature there will be temperature drop in an adiabatic process.
Is in adiabatic process the work done is independent of path?
YES.. By first law of thermodynamics, dQ=dW+dU For adiabatic process dQ=0 dW=-dU Above relation shows that the work done is equal to change in internal energy in magnitude which is the property of the system or point function. Thus work done in adiabatic process is a point function.
When is cryogenic process considered adiabatic?
A process can be considered to be adiabatic if heat loss/transfer is zero, or negligible compared to the system. If the system contains for example, 1 x 10^6 J of heat energy and 3J are lost in a process, the process can be considered adiabatic.
In Adiabatic process how the ideal gases increases it's internal energy?
The first law of thermodynamics states that: DU = DQ + DW where DU is the increase in the internal energy of the gas DQ is the heat supplied to the system and DW is the work done ON the system For an adiabatic process, DQ = 0 Therefore, DU = DW It can be thus easily seen that for the internal to increase (DU +ve), DW must be positive, that is work has to be done on the system (in this case the ideal gas). Hence, the gas should be compressed.
How is heat provided in adiabatic process?
First we measured the temperature of the sample and then give certain amount of heat to it. Then we will measure the final temperature and divide amount of heat supplied to increase in temperature, gives the heat capacity of the sample.
When a gas undergoes adiabatic expansion it gets cooled due to?
It gets cooled because the internal energy of the system decreases.
What is the value of internal energy in a cyclic process in thermodynamics?
Since internal energy is a state function and a cyclic process always returns to the same state (that's how you define a cyclic process), the value of the the internal energy will remain constant. That is not to say that it doesn't change along the cyclic path during the process - just that it always returns to the same value when the cycle is complete.
What are temperature changes that occur even though heat is not added or subtracted?
Temperature changes that occur without any heat addition or subtraction is defined as internal energy. Another term for this occurrence is adiabatic change.
When 430 J of work is done on a system it lost 120 J energy as heat Calculate the value of internal energy change for this process?
The first law of thermodynamics requires that energy input must equal energy output plus energy accumulation. In this case that translates to; 430 J = 120 J + (internal energy change) so Internal energy change = 430 J - 120 J = +310 J (the internal energy increased by 310 Joules)
Why adiabatic curve is steeper than an isothermal curve?
Reason being vaguely adiabatic process is more rapid - process is done so fast that no energy is allowed to enter or exit the system. So P-v variations will be high
