Asystem uses 49 j of energy to do work, and the change in internal energy is 58 j. how much heat was added to the system?
9 j

97 j

107 j

117 j

- 107 J

Solution:- The work done by the system is given as 49 J and the internal energy change is 58 J. It asks to calculate the heat added to the system.

It is based on first law of thermodynamics and the equation used is:

where w is the work done by the system or on the system. q is the heat energy added to the system or released by the system and is the internal energy change.

Since the work is done by the system, the sign of w is negative.

So, w = -49 J

= 58 J

q = ?

Let's plug in the values in the equation:

58 J = q - 49 J

on rearranging this:

q = 58 J + 49 J

q = 107 J

Hence, 107 J of heat is added to the system. Option three is correct.

- "the choice that is not an indicator of a chemical change is "state of matter changes". more common than not, chemical reactions produce energy in the form of light or heat. along with energy, they also produce a new substance called the product that could be in any state of matter (solid, gas, or liquid)."

58750.08068 is the answer i think