methane is used as home fuel find the mass of it which produce 5.6L water pressure

Answer 1

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.