A gas is heated from 203.0 K to 298.0 K and the volume is increased from 24.0 liters to 55.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be? Which Gas Law did you use?
The numerical answer to the question.
An explanation of the correct number of significant figures you will use for the numerical answer

P₂ = 0.6406 atm

Explanation:

Given data:

Initial volume = 24.0 L

Initial pressure = 1.00 atm

Initial temperature = 203.0 K

Final temperature = 298.0 K

Final volume = 55.0 L

Final pressure = ?

Solution:

According to general gas equation:

P₁V₁/T₁ = P₂V₂/T₂

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

P₂ = P₁V₁ T₂/ T₁ V₂  

P₂ = 1 atm × 24.0 L × 298.0 K / 203.0 K × 55.0 L  

P₂ = 7152 atm .L. K / 11165 K.L

P₂ = 0.6406 atm

When we multiply or divide the values the number of significant figures must be equal to the less number of significant figures in given value.

Thus we will include four significant figures in answer because 7152 have four significant figure.

i think the answer is terrae but not 100 percent sure. ▓▬▬ §