4g if impure iron rod was use to stir H2So4 and 1.12dm of H2 was liberated determine the Mass of pure iron rod that reacted with H2SO4
This problem requires knowledge of stoichiometry and the molar mass of iron.
First, let's write the balanced chemical equation for the reaction between iron and sulfuric acid:
Fe + H2SO4 -> FeSO4 + H2
From this equation, we can see that 1 mole of iron reacts with 1 mole of sulfuric acid to produce 1 mole of hydrogen gas. Therefore, we can use the amount of hydrogen produced to determine the amount of iron that reacted:
n(H2) = PV/RT = (1 atm)(0.112 L)/(0.0821 L atm/mol K)(298 K) = 0.00455 moles H2
Since the mole ratio of Fe to H2 is 1:1, we know that 0.00455 moles of iron reacted with the sulfuric acid. Now we need to convert this to mass:
mass(Fe) = n(Fe) x M(Fe)
We don't know the molar mass of the impure iron rod, but we can assume that it is mostly iron and use the molar mass of pure iron (55.85 g/mol) as a reasonable estimate. We can then use the mass of the entire rod, given in the problem, to calculate the mass of pure iron:
mass(pure Fe) = (55.85 g/mol)(0.25 kg) = 14 g
Now we can calculate the number of moles of pure iron that reacted:
n(pure Fe) = mass(pure Fe)/M(pure Fe) = 14 g/55.85 g/mol = 0.25 moles
Since the mole ratio of Fe to H2 is 1:1, we know that 0.25 moles of pure iron reacted with the sulfuric acid. Finally, we can use this to calculate the mass of pure iron that reacted:
mass(pure iron reacted) = n(pure Fe) x M(pure Fe) = 0.25 moles x 55.85 g/mol = 13.96 g
Therefore, approximately 14 grams of pure iron reacted with the sulfuric acid to produce 1.12 dm³ of hydrogen gas.
To determine the mass of the pure iron rod that reacted with H2SO4, we can use the balanced chemical equation and stoichiometry.
The balanced chemical equation for the reaction between iron and sulfuric acid is:
Fe + H2SO4 → FeSO4 + H2
From the equation, we can see that the molar ratio between iron and hydrogen gas is 1:1. This means that for every 1 mole of iron that reacts, 1 mole of hydrogen gas is produced.
First, let's calculate the number of moles of hydrogen gas produced:
Given:
- Volume of hydrogen gas (H2) liberated = 1.12 dm^3
- Pressure and temperature are not provided, but we can assume standard conditions (STP) which is 1 atm and 273 K.
To calculate the number of moles (n) of hydrogen gas, we can use the ideal gas equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in dm^3)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)
Since we are assuming standard conditions, we have:
P = 1 atm
V = 1.12 dm^3
R = 0.0821 L.atm/mol.K
T = 273 K
Plugging in the values, we can solve for n:
1 atm * 1.12 dm^3 = n * 0.0821 L.atm/mol.K * 273 K
1.12 = n * 22.414
n ≈ 0.05 moles (approximately)
Since the molar ratio between iron and hydrogen gas is 1:1, the number of moles of iron that reacted is also approximately 0.05 moles.
Next, we need to determine the molar mass of iron (Fe). The molar mass of iron is 55.85 g/mol.
Finally, we can calculate the mass of the pure iron rod that reacted by multiplying the number of moles of iron by its molar mass:
Mass = number of moles * molar mass
Mass = 0.05 moles * 55.85 g/mol
Mass = 2.79 grams
Therefore, the mass of the pure iron rod that reacted with H2SO4 is approximately 2.79 grams.
To determine the mass of the pure iron rod that reacted with H2SO4, we need to use stoichiometry and the balanced chemical equation.
The balanced chemical equation for the reaction between iron (Fe) and sulfuric acid (H2SO4) is:
Fe + H2SO4 -> FeSO4 + H2
From the equation, we can see that the stoichiometric ratio between iron (Fe) and hydrogen gas (H2) is 1:1. This means that 1 mole of iron will react with 1 mole of hydrogen gas.
Now, let's calculate the number of moles of hydrogen gas. We are given that 1.12 dm^3 of hydrogen gas was liberated. However, we need to convert this volume into moles using the ideal gas law.
The ideal gas law equation is:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
Assuming the reaction occurred at standard temperature and pressure (STP), which is 0 degrees Celsius (273 K) and 1 atm, we can calculate the number of moles of hydrogen gas:
n = PV / RT
= (1 atm) * (1.12 dm^3) / (0.0821 L·atm/(mol·K) * 273 K)
= 0.0516 moles of H2
Since the stoichiometric ratio between iron and hydrogen gas is 1:1, we can conclude that 0.0516 moles of iron also reacted with H2SO4.
To calculate the mass of the pure iron rod, we need to use the molar mass of iron (Fe), which is approximately 55.85 g/mol. We can use the following formula:
Mass = moles * molar mass
= 0.0516 moles * 55.85 g/mol
= 2.876 g
Therefore, the mass of the pure iron rod that reacted with H2SO4 is approximately 2.876 grams.