Answer:
When the pressure and the temperature are increased the volume is 285.7 ml.
Explanation:
We can find the new volume by using the Ideal Gas Law:
[tex] PV = nRT [/tex]
Where:
P: is the pressure
V: is the volume
n: is the number of moles
R: is the gas constant
T: is the temperature
Initially, when V₁ = 200 ml, P₁ = 500 torr and T₁ = 10 °C, we have:
[tex] nR = \frac{P_{1}V_{1}}{T_{1}} [/tex] (1)
And finally, when P₂ = 700 torr and T₂ = 20 °C, we have:
[tex] nR = \frac{P_{2}V_{2}}{T_{2}} [/tex] (2)
By equating (1) with (2):
[tex] \frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}} [/tex]
[tex]V_{2} = \frac{P_{1}V_{1}T_{2}}{T_{1}P_{2}} = \frac{500 torr*200 ml*20 ^{\circ} C}{10 ^{\circ} C*700 torr} = 285.7 ml [/tex]
Therefore, when the pressure and the temperature are increased the volume is 285.7 ml.
I hope it helps you!
