what is volume of hydrogen at STP of hydrogen collected over water at 10 degrees and 105.5 kPa
To calculate the volume of hydrogen at standard temperature and pressure (STP) collected over water at a given temperature and pressure, you need to use the gas laws and account for the vapor pressure of water.
1. Determine the vapor pressure of water at the given temperature:
At 10 degrees Celsius, the vapor pressure of water can be obtained from a water vapor pressure table or by using the Antoine equation. Let's assume it is 1.23 kPa.
2. Calculate the partial pressure of hydrogen:
The total pressure, 105.5 kPa, is composed of the partial pressure of hydrogen and the vapor pressure of water. Therefore, the partial pressure of hydrogen is the difference between the total pressure and the vapor pressure of water:
Partial pressure of hydrogen = Total pressure - Vapor pressure of water
Partial pressure of hydrogen = 105.5 kPa - 1.23 kPa = 104.27 kPa
3. Apply the ideal gas law to find the volume of hydrogen:
The ideal gas law formula is: PV = nRT
Where:
- P is the pressure in Pascals (Pa)
- V is the volume in cubic meters (m^3)
- n is the amount of substance in moles (mol)
- R is the ideal gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin (K)
Convert the given pressure to Pascals:
104.27 kPa = 104.27 × 1000 Pa = 104,270 Pa
Convert the given temperature to Kelvin:
10 degrees Celsius = 10 + 273.15 K = 283.15 K
Rearrange the ideal gas law equation to solve for volume (V):
V = (nRT) / P
Since the amount of substance (n) is not given, we'll assume that 1 mole of hydrogen gas is collected.
Plug in the values into the equation:
V = (1 mol × 8.314 J/(mol·K) × 283.15 K) / 104,270 Pa
4. Calculate the volume of hydrogen:
Now, you can calculate the volume of hydrogen in cubic meters (m^3) using the ideal gas law equation:
V = (1 × 8.314 × 283.15) / 104,270
V ≈ 0.0225 m^3
Therefore, the volume of hydrogen collected over water at 10 degrees Celsius and 105.5 kPa is approximately 0.0225 cubic meters (m^3) at STP.