What would be the original temperature of a gas that has a volume of 2.0 l and a pressure of 2.0 atm and an unknown temperature that the volume increased to 3.5 l in its pressure decreased to 1.0 atm if the final temperature is measured to be 11°c

= 51.57 °C

Explanation:

The combined gas equation shows that P₁V₁/T₁=P₂V₂/T₂ where P represents pressure, V represents volume and T absolute temperature

From the information provided in the question,

Since we are finding the initial or original temperature, we can make T₁ the subject of the formula.

T₁=P₁V₁T₂/P₂V₂

P₁=2.0 ATM

P₂= 1.0 ATM

V₁=2.0 L

V₂= 3.5 L

T₁=?

T₂= (11+273) K=284 K

Using these values in the formula:

T₁= (2.0 ATM × 2.0 L× 284 K)/(1.0 ATM × 3.5 L)

=324.57 K

324.57-273= 51.57 °C

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as in this case where a scientist wants to use a model to present the results of his detailed scientific investigation. he should do it as it will him to make the audience understand the concept in a much better way. also, it can be changed according to new scientific understandings.