Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero)
(a)
Isothermal process q = −w
(b)
Isothermal process q = −w
(c)
Isochoric process 
U = q
(d)
Adiabatic process 
U = −w
Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero)
(a)
Isothermal process q = −w
(b)
Isothermal process q = −w
(c)
Isochoric process U = q
(d)
Adiabatic process U = −w
Question ID - 52428 | SaraNextGen Top Answer
Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero)
(a)
Isothermal process q = −w
(b)
Isothermal process q = −w
(c)
Isochoric process U = q
(d)
Adiabatic process U = −w
|
Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero) |
|||
|
(a) |
Isothermal process q = −w |
(b) |
Isothermal process q = −w |
|
(c) |
Isochoric process |
(d) |
Adiabatic process |
1 Answer
127 votes
Answer Key / Explanation : (d) -
U = q + W
Adiabatic process q = 0
U = W
For isothermal, 
U = 0
For cyclic, 
U = 0
For isochoric, W = 0
127 votes
Answer Link
127