What mass of H2 would be produced by the complete reaction of the iron bar.
Hydrobromic acid dissolves solid iron according to the following reaction:
Fe(s)+2HBr(aq)→FeBr2(aq)+H2(g)
Well, if you give me the mass of the iron bar, I'll bring my trusty chemistry hat and calculate that for you. But be warned, my hat is quite ridiculous-looking.
To determine the mass of H2 produced by the complete reaction of the iron bar, you need to know the mass of the iron bar.
Please provide the mass of the iron bar.
To determine the mass of H2 produced by the complete reaction of the iron bar, you need to know the mass of the iron bar and its molar mass.
Here are the steps to calculate the mass of H2:
1. Determine the molar mass of Fe (iron) and H2 (hydrogen gas). The molar mass of Fe is 55.85 g/mol, and the molar mass of H2 is 2.02 g/mol.
2. Write a balanced equation for the reaction and identify the stoichiometric ratio between Fe and H2. From the given equation:
Fe(s) + 2HBr(aq) → FeBr2(aq) + H2(g)
The stoichiometric ratio between Fe and H2 is 1:1. One mole of Fe reacts with one mole of H2.
3. Calculate the number of moles of Fe in the iron bar. Divide the mass of the iron bar (in grams) by the molar mass of Fe to get the number of moles of Fe.
4. Since the stoichiometric ratio between Fe and H2 is 1:1, the number of moles of H2 produced will be the same as the number of moles of Fe.
5. Multiply the number of moles of H2 by the molar mass of H2 to calculate the mass of H2 produced.
Remember to convert the mass of the iron bar and the mass of H2 to the same units (grams or kilograms) before performing the calculations.
By following these steps, you should be able to determine the mass of H2 produced by the complete reaction of the iron bar.
Answer:
0.226g
Explanation:
Using
mass
=
M
r
×
moles
moles of
F
e
=
6.31
55.8
=
0.113
mol
From the equation, one mole of iron produces one mole of hydrogen gas.
moles of
H
2
=
0.113
mol
mass
H
2
=
0.113
×
2
=
0.226
g