a piece of iron reacts with sulfuric acid and produces 250 dm^3 hydrogen gas at 27 degree celsius temperature and 99.99 kPa. Find out the mass of that piece of iron?
See your other post above.
To find the mass of the iron, we need to use the ideal gas law equation, PV = nRT, where:
P = pressure (99.99 kPa)
V = volume (250 dm³ = 250 L)
n = number of moles of hydrogen gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin (27°C + 273.15 = 300.15 K)
In this case, we're given the pressure, volume, and temperature. We also know that the reaction produces hydrogen gas, and we can use stoichiometry to determine the number of moles of hydrogen produced.
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 is 1:1. This means that for every one mole of iron, one mole of hydrogen gas is produced.
Now let's calculate the number of moles of hydrogen gas using the ideal gas law equation:
PV = nRT
n = PV / RT
= (99.99 kPa) * (250 L) / (0.0821 L·atm/(mol·K)) * (300.15 K)
≈ 102.53 moles
Since the molar ratio between iron and hydrogen is 1:1, the number of moles of iron is also approximately 102.53 moles.
To calculate the mass of the iron, we need to know the molar mass of iron (Fe), which is approximately 55.85 g/mol.
Mass of iron = number of moles of iron * molar mass of iron
= 102.53 moles * 55.85 g/mol
≈ 5729.65 g
Therefore, the mass of the iron piece is approximately 5729.65 grams.