Iron reacts with hydrochloric acid to produce iron (2) chloride and hydrogen gas.Fe (s)+ 2 HCL (aq) -FeCl2 (aq) + H2 (g).The hydrogen gas from the reaction 2.2g of iron with excess acid is collected in a 10L flask at 25 degrees celcius. What is the pressure of the hydrogen gas in the flask?
First off, I don't know what iron(2) chloride is. I assume you meant iron(II) chloride.
1. You have the balanced equation.
2. Convert 2.2 g Fe to moles. #moles = g/molar mass.
3. Using the coefficients in the balanced equation, convert moles Fe to moles H2.
4. Now use PV=nRT to calculate P.
To find the pressure of the hydrogen gas in the flask, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles of the gas
R = gas constant (0.0821 L.atm/(mol.K))
T = temperature of the gas (in Kelvin)
First, let's calculate the number of moles of hydrogen gas using the given mass of iron. We will need the molar mass of iron.
The molar mass of iron (Fe) is:
1 mole of Fe = 55.845 g
Given mass of Fe = 2.2 g
Number of moles of Fe = mass of Fe / molar mass of Fe
Number of moles of Fe = 2.2 g / 55.845 g/mol
Next, we need to find the moles of hydrogen gas produced. The stoichiometry of the reaction tells us that 1 mole of Fe reacts to produce 1 mole of H2 gas. So, the number of moles of H2 gas produced is equal to the moles of Fe:
Number of moles of H2 gas = 2.2 g / 55.845 g/mol
Now, we can substitute the values we have into the ideal gas law equation and solve for P:
P * V = n * R * T
Given V = 10 L and T = 25°C = 25 + 273.15 K
P * 10 = (2.2 g / 55.845 g/mol) * 0.0821 L.atm/(mol.K) * (25 + 273.15) K
Simplifying:
10P = 0.0393 mol * 0.0821 L.atm/(mol.K) * 298.15 K
10P = 1.017 L.atm
Dividing both sides by 10:
P = 1.017 L.atm / 10
P = 0.1017 atm
Therefore, the pressure of the hydrogen gas in the flask is approximately 0.1017 atm.
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.