Question

330 J of energy is transferred to a system consisting of 2.0 moles of an ideal gas. If the volume of this gas stays at a constant 4.4 L, calculate the change in internal energy of the gas.

Answer 1

The change in internal energy for the ideal gas at constant volume is equal to the heat transferred to the system, which in this case is 330 J.

Step-by-step explanation:

To calculate the change in internal energy of an ideal gas at constant volume, we need to apply the first law of thermodynamics which is:

(Delta U = Q - W)

Where:

• (Delta U) is the change in internal energy
• Q is the heat transferred to the system
• W is the work done by the system

Since the volume of the gas does not change, the work done by the system is zero (W=0) because work is defined by (W = P \Delta V\), and when \(\Delta V = 0\), no work is performed.

Thus the equation simplifies to:

(Delta U = Q)

In this student's question, 330 J of energy is transferred to the system (Q),

so the change in internal energy (Delta U) would also be 330 J since no work is done on or by the system.