Final answer:
The internal energy of 6.00 mol of an ideal monatomic gas at 200°C is approximately 118.7 J. The correct answer is (a) 120 J.
Step-by-step explanation:
The internal energy of 6.00 mol of an ideal monatomic gas at 200°C can be calculated using the equation:
ΔU = nCvΔT
Where ΔU is the change in internal energy, n is the number of moles of gas, Cv is the molar heat capacity at constant volume, and ΔT is the change in temperature.
Since the gas is ideal and monatomic, Cv = (3/2)R, where R is the gas constant. The change in temperature is given by ΔT = (200 - 0) °C = 200 K. Therefore, the change in internal energy is:
ΔU = (6.00 mol)(3/2)(8.314 J/mol*K)(200 K) = 118.7 J
Therefore, the internal energy of the gas is approximately 118.7 J.