Final answer:
The change in internal energy of the gas is 970 J.
Step-by-step explanation:
To determine the change in internal energy (ΔU) of the ideal gas, we can use the first law of thermodynamics, which states that ΔU = Q - W, where Q is the heat added to the system and W is the work done by the system. In this case, the experimenter adds 970 J of heat (Q) to the gas.
Assuming the process is carried out at constant volume (no work done, W = 0), the change in internal energy simplifies to ΔU = Q. Therefore, the change in internal energy is 970 J.
This result signifies that the internal energy of the ideal gas increases by 970 J as a result of the added heat. It's crucial to note that the ideal gas law and the assumption of constant volume simplify the calculation in this scenario.