Answer:
379.5 joules (J) of energy were made unavailable for useful work as a result of this irreversible process.
Step-by-step explanation:
To calculate the amount of energy made unavailable for useful work during the irreversible process, we can use the formula:
ΔS_universe = ΔS_system + ΔS_environment
where:
ΔS_universe = Change in entropy of the universe
ΔS_system = Change in entropy of the system
ΔS_environment = Change in entropy of the environment
In this case, the change in entropy of the universe (ΔS_universe) is given as 1.65 J/K. The temperature of the environment (T_environment) is given as 230 K.
Since the process is irreversible, the change in entropy of the system (ΔS_system) will be zero, as the system is not in equilibrium with its surroundings during the process.
Now, we can calculate the change in entropy of the environment (ΔS_environment) using the formula:
ΔS_environment = ΔQ / T_environment
where:
ΔS_environment = Change in entropy of the environment
ΔQ = Heat exchanged with the environment
T_environment = Temperature of the environment
Since the change in entropy of the system is zero, all the energy absorbed as heat from the environment (ΔQ) is converted into an increase in entropy in the environment. So:
ΔS_environment = 1.65 J/K
ΔQ = ?
Now, rearrange the formula to solve for ΔQ:
ΔQ = ΔS_environment * T_environment
ΔQ = 1.65 J/K * 230 K
ΔQ = 379.5 J
Therefore, 379.5 joules (J) of energy were made unavailable for useful work as a result of this irreversible process.