El metal Mg reacciona con el Hcl para producir gas Hidrógeno Mg +2HCl---MgCl2 + H2. ¿Qué volumen en Litros de H2 en condiciones STP se liberan cuando reaccionan 8.25g de Mg? * 8.60L 6.60L 7.60L 16.60L

7.60 L of hydrogen gas will be liberated.

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

The equation used is:

   ......(1)

Given mass of Mg = 8.25 g

Molar mass of Mg = 24.305 g/mol

Plugging values in equation 1:

The given chemical equation follows:

By the stoichiometry of reaction:

If 1 mole of magnesium produces 1 mole of hydrogen gas

So, 0.340 moles of magnesium will be produce = of hydrogen gas

At STP conditions:

1 mole of a gas occupies 22.4 L of volume

So, 0.340 moles of hydrogen gas will occupy = of hydrogen gas

Hence, 7.60 L of hydrogen gas will be liberated.

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.