What is the Volume of the water vapour if 3.2 grams of water vapour is observed at 22 C
and 125 kPa. ? R = 8.31 L kPa/ K mol
Given:
Mass of water is 3.2 g
Molar mass of water is 18.0153 g mol−1
T = 22°C + 273.15 = 295.15 K
P = 125 kPa
R = 8.31 L kPa K−1 mol−1
Solution:
Moles = Mass / Molar mass
Therefore,
Moles of water = (3.2 g) / (18.0153 g mol−1) = 0.1776 mol
n = 0.1776 mol
The ideal gas law relates the amount of gas present to its pressure, volume, and temperature.
The ideal gas law is written as PV = nRT,
where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.
Rearrange the equation to solve for V:
V = nRT / P
Plug in the numbers:
V = (0.1776 mol × 8.31 L kPa K−1 mol−1 × 295.15 K) / (125 kPa) = 3.4848 L = 3.5 L
V = 3.5 L
Answer: The volume of the water vapour is 3.5 liters
Comments
Leave a comment