Question

80.0 ML of fluorine gas is held in a flexible vessel at STP. If the vessel is transported to the surface of Venus where the pressure is 92.0 ATM and The temperature is 460 Celsius what is the new volume of the gas in millimeters

Answer 1

Answer:

The new volume of the gas is 2.33 mL

Explanation:

Step 1: data given

Volume of the fluorine gas = 80.0 mL = 0.080 L

STP = 1 atm and 273 K

The new pressure is 92.0 atm

The new temperature = 460 °C = 733 K

Step 2: Calculate the new volume

P1*V1 / T1  = P2 *V2 / T2

⇒with P1 = the initial pressure of the fluorine gas = 1 atm

⇒with V1 = the initial volume of the fluorine gas = 0.080 L

⇒with T1 = the initial temperature of the fluorine gas = 273 K

⇒with P2 = the new pressure of the gas = 92.0 atm

⇒with V2 = the new volume of the gas = TO BE DETERMINED

⇒with T2 = the new temperature of the gass = 733 K

(1 atm * 0.080 L)/273 K = (92.0 atm * V2) / 733 K

2.93 * 10^-4 = (92.0 atm * V2) / 733 K

0.214769 = (92.0 atm * V2)

V2 = 0.214769 / 92.0

V2 = 0.00233 L = 2.33 mL

The new volume of the gas is 2.33 mL

Answer 2

Answer:

2.33 mL

Explanation:

Given data

• Initial pressure (P₁): 1 atm (Standard pressure)

• Initial volume (V₁): 80.0 mL

• Initial temperature (T₁): 273.15 K (Standard temperature)

• Final pressure (P₂): 92.0 atm

• Final volume (V₂): ?

• Final temperature (T₂): 460°C + 273.15 = 733 K

We can find the new volume using the combined gas law.

$\frac{P_1 \times V_1 }{T_1} = \frac{P_2 \times V_2 }{T_2}\\V_2 = \frac{P_1 \times V_1 \times T_2 }{T_1 \times P_2}\\V_2 = \frac{1 atm \times 80.0mL \times 733K }{273.15K \times 92.0atm}=2.33 mL$