Final answer:
To solve this problem, you need to calculate the change in temperature, the specific heat capacity at constant pressure, and then use the formula Q = n * Cp * ΔT to calculate the heat transferred. So, the correct option is (a) 72 J.
Step-by-step explanation:
The specific heat capacity of an ideal monatomic gas at constant volume (Cv) is given by the formula Cv = (3/2)R, where R is the gas constant.
To determine the heat transferred during an isobaric expansion, we use the formula Q = n * Cp * ΔT, where Q is the heat transferred, n is the number of moles of gas, Cp is the specific heat capacity at constant pressure, and ΔT is the change in temperature.
In this case, the gas expands isobarically to triple its volume, so the final volume is 3 times the initial volume. Since the process is isobaric, the pressure remains constant at 1.00 atm.
The change in temperature can be calculated using the ideal gas law: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin.
Calculate the change in temperature (ΔT) using the ideal gas law.
Calculate the specific heat capacity at constant pressure (Cp) using the formula Cp = (5/2)R.
Substitute the values into the formula Q = n * Cp * ΔT to calculate the heat transferred.
Using the given values, we can calculate the heat transferred.
So, the correct option is (a) 72 J.