Answer:
n = 1.9 ×10⁻⁵ mol
Explanation:
Given data:
Volume of hydrogen gas = 455 mm
Pressure of hydrogen gas = 101.3 kpa
Temperature = 29.1°C
Partial pressure of water vapor = 4.0 kpa
Number of moles of hydrogen gas = ?
Solution:
First of all we will convert the units.
Pressure of hydrogen gas = 101.3 kpa= 101.3/101 = 1 atm
Partial pressure of water vapor = 4.0 kpa = 4.0/ 101 = 0.04 atm
Temperature = 29.1 + 273 = 302.1 K
Volume of hydrogen gas = 455 / 1×10⁶ = 0.000455 L
Now we will calculate the total pressure.
Total pressure = Partial pressure of hydrogen gas + partial pressure of water vapors
Total pressure = 1 atm + 0.04 atm
Total pressure = 1.04 atm
Now we will calculate the number of moles;
PV = nRT
n = PV/RT
n = 1.04 atm × 0.000455 L / 0.0821 atm.L / mol.K × 302.1 K
n = 0.00047 /24.80/mol
n = 1.9 ×10⁻⁵ mol
Answer:
First, calculate the partial pressure of hydrogen by subtracting the total pressure of the hydrogen–water vapor mixture from the partial pressure of water vapor:
101.3 kPa − 4.0 kPa = 97.3 kPa.
Convert the temperature to kelvins:
29.1°C + 273.15 = 302.25 K.
Convert milliliters to liters by dividing by 1,000 to get 0.455 L.
Since the pressure is in kilopascals, use the R value 8.314 .
Now substitute the known values into the ideal gas equation:
n =
n =
n =
n = 0.0176176 mol
n = 0.0176 mol
Explanation:
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