To find the pressure of the hydrogen gas in the flask, we need to use the ideal gas law equation:
PV = nRT
Where:
P = Pressure of the gas
V = Volume of the gas
n = Number of moles of the gas
R = Ideal gas constant (0.0821 L·atm/mol·K)
T = Temperature in Kelvin
First, let's calculate the number of moles of hydrogen gas produced in the reaction.
To do this, we need to find the molar mass of iron (Fe). The atomic mass of iron is 55.85 g/mol.
Given:
Mass of iron (Fe) = 2.2 g
Moles of iron (Fe) = mass / molar mass
Moles of iron (Fe) = 2.2 g / 55.85 g/mol ≈ 0.039 mol
According to the balanced chemical equation, the stoichiometry between iron (Fe) and hydrogen gas (H2) is 1:1. Therefore, the number of moles of hydrogen gas produced will also be approximately 0.039 mol.
Next, we convert the given temperature from degrees Celsius to Kelvin.
Given:
Temperature = 25 degrees Celsius
Temperature in Kelvin = 25 + 273.15 K ≈ 298.15 K
Now we can substitute the values into the ideal gas law equation.
PV = nRT
P * 10 L = 0.039 mol * 0.0821 L·atm/mol·K * 298.15 K
To solve for P, divide both sides of the equation by 10 L:
P = (0.039 mol * 0.0821 L·atm/mol·K * 298.15 K) / 10 L
P ≈ 0.960 atm
Therefore, the pressure of the hydrogen gas in the flask is approximately 0.960 atm.