Final answer:
To increase the temperature of 1.3 g of argon by 100°C at constant volume, 0.40014 L·atm of heat is required.
Step-by-step explanation:
To calculate the heat required, we can use the equation Q = nCΔT, where Q is the heat, n is the number of moles of the gas, C is the molar heat capacity at constant volume, and ΔT is the change in temperature.
First, we need to find the number of moles of argon. Since the molar mass of argon is 39.95 g/mol, we can use the equation n = m/M, where m is the mass of the gas and M is the molar mass. Plugging in the values, we get n = 1.3 g / 39.95 g/mol = 0.03254 mol.
The molar heat capacity at constant volume (Cv) for an ideal gas is 3/2R, where R is the gas constant. In this case, we can use the value of R = 0.0821 L·atm/(mol·K). Therefore, Cv = 3/2 * 0.0821 L·atm/(mol·K) = 0.12315 L·atm/(mol·K).
Now, we can calculate the heat using the equation Q = nCΔT. Plugging in the values, we get Q = 0.03254 mol * 0.12315 L·atm/(mol·K) * 100 °C = 0.40014 L·atm.