Final answer:
Heating 6.0 mol of argon gas sealed at 1.0 atm to triple its pressure will also triple the gas's temperature, assuming the volume remains constant, according to the ideal gas law.
Step-by-step explanation:
When 6.0 mol of argon gas are sealed in a container at 1.0 atm and then the container is heated until the pressure triples, we are dealing with an application of the ideal gas law. This law is represented by the equation PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. Since the pressure triples and the amount of gas and the volume remain constant, the absolute temperature must also triple to maintain the direct relationship as described by Charles's Law (a part of the ideal gas law). Therefore, when heating the argon gas for the pressure to triple, the temperature would also have to triple assuming the volume is constant.