Fe(S)+ 2 HCl(ag) --> FeCL2(ag)+ H2(g
What mass of H2 (g) is produced from the reaction of 5.2 Fe(s) with excess hydrochloric acid?
Here is a simple stoichiometry problem I've posted as an example. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
.094
To find the mass of H2 gas produced, we need to use stoichiometry, which is a way to relate the amounts of different substances in a chemical reaction.
The balanced chemical equation for the reaction is:
Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g)
From the equation, we can see that the molar ratio between Fe(s) and H2(g) is 1:1. This means that for every 1 mole of Fe(s) reacted, 1 mole of H2(g) is produced.
To solve this problem, we need to follow these steps:
Step 1: Calculate the molar mass of Fe(s)
The molar mass of iron (Fe) is approximately 55.85 g/mol. Therefore, the molar mass of Fe(s) is 55.85 g/mol.
Step 2: Calculate the number of moles of Fe(s) reacted
We are given that the mass of Fe(s) reacted is 5.2 g. To calculate the number of moles, we use the formula:
Number of moles = Mass / Molar mass
Number of moles = 5.2 g / 55.85 g/mol
Number of moles ≈ 0.093 mol
Step 3: Calculate the mass of H2(g) produced
Since the molar ratio between Fe(s) and H2(g) is 1:1, the number of moles of H2(g) produced is also 0.093 mol.
To find the mass of H2(g), we use the formula:
Mass = Number of moles × Molar mass
The molar mass of hydrogen (H2) is approximately 2.02 g/mol. Therefore, the mass of H2(g) produced is:
Mass = 0.093 mol × 2.02 g/mol
Mass ≈ 0.188 g
Therefore, approximately 0.188 grams of H2 gas is produced from the reaction of 5.2 grams of Fe(s) with excess hydrochloric acid.