Hydrogen gas can be produced by the reaction of magnesium metal with hydrochloric acid as shown in the following chemical reaction. Identify the limiting reagent when 6.00 grams of HCl reacts with 5.00 grams of Mg.

HCI is the answer

To identify the limiting reagent in a chemical reaction, we need to compare the number of moles of each reactant and see which one runs out first.

To do this, we can follow these steps:

1. Write the balanced chemical equation:
Mg + 2HCl → MgCl2 + H2

2. Calculate the molar mass of each reactant:
The molar mass of HCl is 1.008 g/mol for hydrogen and 35.45 g/mol for chlorine.
So, the molar mass of HCl is 1.008 + 35.45 = 36.458 g/mol.

The molar mass of Mg is 24.31 g/mol.

3. Convert the mass of each reactant to moles:
Moles = mass / molar mass

For HCl: Moles of HCl = 6.00 g / 36.458 g/mol
For Mg: Moles of Mg = 5.00 g / 24.31 g/mol

Moles of HCl ≈ 0.165 mol
Moles of Mg ≈ 0.205 mol

4. Determine the stoichiometric ratio of the reactants:
From the balanced chemical equation, we see that the ratio between HCl and Mg is 2:1. This means that for every 2 moles of HCl, 1 mole of Mg is needed.

5. Compare the moles of HCl and Mg:
Since we have fewer moles of HCl (0.165 mol) compared to Mg (0.205 mol), HCl is the limiting reagent.

Therefore, the limiting reagent is HCl.

So you have

Mg + 2HCl = MgCl2 + H2
you have 5/24.3 moles of Mg
you have 6/36.5 moles of HCl
so, which will be used up first?

dk