Final answer:
a. 275 K Using the ideal gas law (PV = nRT), the temperature of a gas with 1.62 atm pressure, 22.4 L volume, and 1.60 moles was calculated to be 275 K.
Step-by-step explanation:
To answer the student's question, we need to use the ideal gas law, which is PV = nRT. The variables P, V, n, and T represent the pressure, volume, number of moles, and temperature of the gas, respectively, while R is the ideal gas constant. Given the pressure (P) as 1.62 atm, volume (V) as 22.4 L, and number of moles (n) as 1.60, our aim is to solve for the temperature (T) in Kelvins (K).
The ideal gas constant (R) can be used in various units, but for this problem, we will use 0.08206 (L.atm)/(K.mol) since we're working with atmospheres and liters. The temperature (T) in Kelvin can be found by rearranging the ideal gas law to T = PV/(nR). Substituting the known values, we get:
T = (1.62 atm * 22.4 L) / (1.60 mol * 0.08206 L.atm/(K.mol)) = 275 K
The correct answer is 275 K, which corresponds to answer choice (a).