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A reaction at 12.0 °C evolves 358, mmol of sulfur hexafluoride gas. Calculate the volume of sulfur hexafluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits. volume: LL

Respuesta :

Answer:

The volume of the gas is 8.37 L

Explanation:

Step 1: Data given

Temperature = 12.0 °C

Moles sulfur hexafluoride gas = 358 mmol = 0.358 mol

Pressure = 1 atm

Step 2: Calculate volume

p*V = n*R*T

⇒ with p = the pressure = 1 atm

⇒ with V = The volume = TO BE DETERMINED

⇒ with n = moles of sulfur hexafluoride gas

⇒ with R = the gas constanr = 0.08206 L*atm/mol*K

⇒ with T = The temperature = 12.0 °C = 285 K

V = (n*R*T)/p

V = ( 0.358 * 0.08206 * 285) / 1

V = 8.37 L

The volume of the gas is 8.37 L

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