Ishwar S. answered • 06/28/18

Tutor

5
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University Professor - General and Organic Chemistry

Hello Alyssa

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 (P

_{i}) = 500 atm and the initial temperature (T_{i}) = 298 K. We need to determine the pressure (P_{f}) of the final state when the temperature (T_{f}) is increased to 1000 K.The Gay-Lusaac's equation is:

P

*/ T*_{i}*= P*_{i}*/ T*_{f}_{f}Rearrange to solve for P

*, you get*_{f}P

_{f}= P

*x Tf / T*

_{i}_{i}= 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.