Question

A gas sample is heated from -20.0°C to 57.0°C and the volume is increased from 2.00 L to 4.50 L. If the initial pressure is 0.140 atm, what is the final pressure? Select one: a. 0.0477 atm b. –0.177 atm c. 0.411 atm d. 0.242 atm e. 0.0811 atm

Answer 1

Answer:

The answer is e.

Explanation:

We take:

$T_{1}=253K$

$V_{1}=2.00 l$

$P_{1}=0.14atm$

$V_{2}=4.50 l$

$T_{2}=330K$

Taking the gas as an ideal gas, we can use the ideal gas law:

$\frac{PV}{nRT}$

⇒ $n=\frac{P_{1}V_{1}}{RT_{1}}$ ⇒ $n=0.013mol$

Then:

$P_{2}=\frac{nRT_{2}}{V_{2}}$ ⇒ $P_{2}=0.0811 atm$

Taking R=0.08205atmL/molK.