This question deals with Gay-Lusaac's Law, which states that the pressure (P) of a gas varies directly with the Kelvin temperature (T).
P ∝ T
In your question, you can see that the temperature is increasing from 298 K to 1000 K. The effect will be a significant increase in the pressure, which can be dangerous depending on the equipment being used.
In your question, you have an initial state where the initial pressure (Pi) = 500 atm and the initial temperature (Ti) = 298 K. We need to determine the pressure (Pf) of the final state when the temperature (Tf) is increased to 1000 K.
The Gay-Lusaac's equation is:
Pi / Ti = Pf / Tf
Rearrange to solve for Pf, you get
Pf = Pi x Tf / Ti = 500 atm x 1000 K / 298 K = 1678 atm
The situation is dangerous because the pressure has increased to 1678 atm, which is more than 3 times the initial pressure.
Hope that above is helpful.