To calculate the value of \( E \) (the internal energy of the system), we can use the first law of thermodynamics, which states:
\[ \Delta U = Q + W \]
Where:
- \( \Delta U \) is the change in internal energy (which we can denote as \( E \)).
- \( Q \) is the heat added to the system (if the system loses heat, \( Q \) will be negative).
- \( W \) is the work done on the system (if work is done on the system, \( W \) is positive).
In this case:
- The system loses 31 J of heat, so \( Q = -31 , \text{J} \).
- The system has 150 J of work performed on it by the surroundings, so \( W = 150 , \text{J} \).
Now we can substitute these values into the equation:
\[ E = Q + W \] \[ E = (-31 , \text{J}) + (150 , \text{J}) \] \[ E = -31 + 150 \] \[ E = 119 , \text{J} \]
Thus, the value of \( E \) is \( 119 , \text{J} \).
2 answers