Question

A gas is heated from 213.0 K to 298.0 K and the volume is increased from 14.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 3.15 atm, what would the final pressure be?
Include the following with your answer:

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.

Answer 1

Answer:

The answer is ""

Explanation:  

Given:

$V_1= 14.0\ L\\\\P_1= 3.15\ atm\\\\T_1 = 213.0 \ K\\\\T_2= 298.0\ K\\\\V_2= 35.0\ L\\\\P_2 = ?$

Using formula:

$\to \frac{P_1V_2}{T_1} = \frac{P_2V_2}{T_2}\\\\P_2 = \frac{P_1V_1 T_2}{T_1 V_2}$

     $= \frac{3.15 \times 14.0 \times 298.0}{213.0 \times 35.0} \\\\= \frac{13141.0}{7455} \\\\=1.7627\\\\=1.8\ atm$