calculate the amount of hydrogen gas involved if ferrous + 2hcl = ferrous choloride + h2 if 55 gramme iron is reacting with 36.5 hydrochloric acid .

Don't you mean

Fe + 2HCl -> FeCl2 + H2 ?
55g Fe is 0.984 moles
36.5 g HCl is 1.000 moles

HCl is slightly in excess of stoichiomentric.

0.984 moles of HCl are evolved.
That is 22 liters at STP

To calculate the amount of hydrogen gas involved in the reaction, we need to use the concept of stoichiometry. Stoichiometry allows us to determine the relative quantities of reactants and products involved in a chemical reaction.

First, let's write down the balanced chemical equation for the reaction:

Fe + 2HCl → FeCl2 + H2

According to the balanced equation, 1 mole of iron (Fe) reacts with 2 moles of hydrochloric acid (HCl) to form 1 mole of ferrous chloride (FeCl2) and 1 mole of hydrogen gas (H2).

Now, let's calculate the moles of iron and hydrochloric acid:

Molar mass of iron (Fe) = 55.845 g/mol
Molar mass of hydrochloric acid (HCl) = 36.461 g/mol

Moles of iron = Mass of iron / Molar mass of iron
= 55 g / 55.845 g/mol
= 0.984 mol (approx.)

Moles of hydrochloric acid = Mass of HCl / Molar mass of HCl
= 36.5 g / 36.461 g/mol
= 1 mol (approx.)

From the balanced equation, we know that the ratio of moles of iron to moles of hydrogen gas is 1:1. Therefore, the number of moles of hydrogen gas produced is also 0.984 mol.

Finally, if we want to convert the moles of hydrogen gas to grams, we can use the molar mass of hydrogen (H2), which is 2 g/mol.

Mass of hydrogen gas = Moles of H2 * Molar mass of H2
= 0.984 mol * 2 g/mol
= 1.968 g

Therefore, the amount of hydrogen gas involved in the reaction is approximately 1.968 grams.

To calculate the amount of hydrogen gas (H2) that is involved in the reaction, we need to determine the stoichiometry of the reaction. The balanced equation for the reaction is:

Fe + 2HCl -> FeCl2 + H2

From the balanced equation, we can see that for every 1 mole of Fe reacted, 1 mole of H2 gas is produced.

First, we need to determine the number of moles of the reactants using their molar masses.

1. For iron (Fe):
Molar mass of Fe = 55.845 g/mol
Number of moles of Fe = Mass / Molar mass
Number of moles of Fe = 55 g / 55.845 g/mol
Number of moles of Fe = 0.9848 mol

2. For hydrochloric acid (HCl):
Molar mass of HCl = 1.00784 g/mol + 35.453 g/mol
Molar mass of HCl = 36.46084 g/mol
Number of moles of HCl = Mass / Molar mass
Number of moles of HCl = 36.5 g / 36.46084 g/mol
Number of moles of HCl = 1 mol

Since the stoichiometry ratio between Fe and H2 is 1:1, the number of moles of hydrogen gas produced will be equal to the number of moles of Fe.

Number of moles of H2 = 0.9848 mol

Finally, to calculate the amount of hydrogen gas involved, we can multiply the number of moles of H2 by its molar mass.

Molar mass of H2 = 2.01588 g/mol
Amount of H2 = Number of moles of H2 * Molar mass of H2
Amount of H2 = 0.9848 mol * 2.01588 g/mol
Amount of H2 = 1.981 g

Therefore, the amount of hydrogen gas involved in the reaction is approximately 1.981 grams.