Final answer:
The work done and the heat transferred to an ideal gas during isothermal expansion are theoretically equal, given by the equation W = nRT · ln(V2/V1) where n is the number of moles, R the gas constant, T the absolute temperature, and V2 and V1 the final and initial volumes. Without initial volume or pressure data, these values cannot be calculated here.
Step-by-step explanation:
When dealing with an ideal gas, the concepts of pressure, volume, and temperature are essential to understanding its behavior. For an isothermal expansion, the temperature of the gas remains constant.
According to the first law of thermodynamics, the change in the internal energy of an ideal gas in an isothermal process is zero, which implies that the work done by the gas (W) is equal to the heat added to the system (Q).
The work done by an ideal gas during an isothermal expansion can be calculated using the formula W = nRT · ln(V2/V1), where n is the number of moles, R the gas constant, T the absolute temperature, and V2 and V1 are the final and initial volumes, respectively. Here, we don't have values for initial volume or pressure to calculate the work or heat.