Okay, here are the steps to solve this problem:
1) We are given the pressure (P) of argon at 2.17 atm and temperature (T) of 32°C.
2) We need to find the temperature at which the pressure increases to 2.83 atm.
3) For an ideal gas like argon, the pressure and temperature are directly proportional. We can use Boyle's Law:
P proportional to T (at constant volume)
4) Set up a proportion:
(2.17 atm) / (32°C) = (2.83 atm) / (x °C)
5) Solve for x:
x = (2.83 atm * 32°C) / (2.17 atm)
x = 43°C
Therefore, the argon gas sample will reach a pressure of 2.83 atm at 43°C.
Let me know if you have any other questions!