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.

im pretty sure its b

definition

                    entropy is a measure of the randomness or the extent of disorder of a chemical process.

                      enthalpy is a measure of the heat change of a reaction occurring at a constant pressure.

measurement units:

                        entropy is measured in joule per kelvin (jk⁻¹)   whereas enthalpy is measured in joule per mole (jmol⁻¹)

requirements:

                            entropy has no requirements or limits, and its change is measured by the division between the heat change of the chemical process and the temperature.

                              in contrast, enthalpy can only be related to the heat change of the reaction under standard conditions.