Question

Calculate the amount of hydrogen under normal conditions, which is released under the influence of excess hydrochloric acid on 11.2 g of iron. The interaction proceeds according to the equation: Fe + 2HCl → FeCl2 + H2.

Answer 1

Ответ:

Fe+2HCl=>FeCl2+H2

11,2g (Fe)------xmol (H2)

56g (Fe)-------1 mol

x=(11,2×1)/56=0,2mol (H2)

Answer: 0,2 mol H2

Answer 2

To calculate the amount of hydrogen gas released under the influence of excess hydrochloric acid on 11.2 g of iron, we can use stoichiometry and the given balanced chemical equation.

The balanced equation for the reaction is:

Fe + 2HCl → FeCl2 + H2

From the equation, we can see that 1 mole of iron (Fe) reacts with 2 moles of hydrochloric acid (HCl) to produce 1 mole of hydrogen gas (H2).

To determine the amount of hydrogen gas produced, we need to convert the mass of iron (Fe) to moles using its molar mass. The molar mass of iron is 55.85 g/mol.

First, calculate the number of moles of iron (Fe):

moles of Fe = mass of Fe / molar mass of Fe moles of Fe = 11.2 g / 55.85 g/mol

Next, use the stoichiometry of the balanced equation to determine the number of moles of hydrogen gas (H2) produced:

moles of H2 = moles of Fe

Finally, convert the number of moles of hydrogen gas (H2) to grams using its molar mass. The molar mass of hydrogen is 2.02 g/mol.

mass of H2 = moles of H2 * molar mass of H2

By substituting the values into the equation, we can calculate the amount of hydrogen gas released:

moles of H2 = 11.2 g / 55.85 g/mol moles of H2 = 0.2 mol

mass of H2 = 0.2 mol * 2.02 g/mol mass of H2 = 0.404 g

Therefore, under normal conditions, approximately 0.404 grams of hydrogen gas will be released when 11.2 grams of iron reacts with excess hydrochloric acid.