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An 0.539 mol sample of helium gas at a temperature of 10.0°C is found to occupy a volume of 25.4 liters. The pressure of this gas sample is atm.

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Answer:

1.354 atm

Explanation:

We used a formula to find the pressure of helium gas. Imagine it like this:

Pressure = (Amount of helium x Gas constant x Temperature) / Volume

Amount of helium = 0.539 moles

Gas constant = 0.0821 L·atm/mol·K

Temperature = 10.0°C + 273.15 = 283.15 K

Volume = 25.4 L

Plug in these values:

Pressure = (0.539 x 0.0821 x 283.15) / 25.4

Pressure ≈ 1.354 atm

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