methane is used as home fuel find the mass of it which produce 5.6L water pressure
To find the mass of methane that produces 5.6L of water pressure, we need to use the ideal gas law equation:
PV = nRT
Where:
P = water pressure (in Pa)
V = volume of methane (in m^3)
n = number of moles of methane
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin)
Since we are given the volume of water pressure in liters, we need to convert it to cubic meters:
5.6L = 5.6 * 10^-3 m^3
Now we can rearrange the equation to solve for n (number of moles):
n = PV / RT
We'll use the following values:
P = 5.6 * 10^5 Pa (1 Pa = 1 N/m^2)
V = 5.6 * 10^-3 m^3
R = 8.314 J/(mol·K)
T = room temperature = 25°C = 298K
n = (5.6 * 10^5 Pa * 5.6 * 10^-3 m^3) / (8.314 J/(mol·K) * 298K)
n = 10.854 mol
Now, we need to find the molar mass of methane:
CH4:
- Carbon has a molar mass of 12.01 g/mol
- Hydrogen has a molar mass of 1.008 g/mol
(4 * 1.008 g/mol) + (12.01 g/mol) = 16.043 g/mol
Finally, we can calculate the mass of methane:
mass = n * molar mass
mass = 10.854 mol * 16.043 g/mol
mass ≈ 173.97 g
Therefore, the mass of methane that produces 5.6L of water pressure is approximately 173.97 grams.