Calculate how many cm3 of 1M HCl is necessary to dissolve 1g of magnesium ribbon
Mg + 2HCl ==> H2 + MgCl2
mols Mg = grams/atomic mass = ?
Using the coefficients in the balanced equation, convert mols Mg to mols HCl.That's 1 mol Mg = 2 mol HCl
Now M HCl = mols HCl/L HCl. You know mols HCl and M HCl, solve for L HCl and convert to cc3 (mL).
500cm^3
To solve this problem, we need to use the chemical equation for the reaction between magnesium and hydrochloric acid:
Mg + 2HCl → MgCl2 + H2
From the balanced chemical equation, we can see that one mole of magnesium reacts with two moles of hydrochloric acid to produce one mole of magnesium chloride and one mole of hydrogen gas.
First, we need to determine the moles of magnesium, given the mass of magnesium ribbon. The molar mass of magnesium (Mg) is approximately 24.31 g/mol.
Moles of magnesium = mass of magnesium (g) / molar mass of magnesium (g/mol)
= 1 g / 24.31 g/mol
≈ 0.041 moles
Since the stoichiometry of the reaction tells us that 1 mole of magnesium reacts with 2 moles of hydrochloric acid, we can determine the moles of hydrochloric acid required.
Moles of hydrochloric acid = 2 * moles of magnesium
= 2 * 0.041 moles
≈ 0.082 moles
Now, we can use the concentration of the hydrochloric acid (1 M) to calculate the volume required.
Concentration (M) = moles of solute / volume of solution (L)
Volume of solution (L) = moles of solute / concentration (M)
= 0.082 moles / 1 M
≈ 0.082 L
Finally, we can convert the volume from liters to cm3.
1 L = 1000 cm3
Volume of solution (cm3) = 0.082 L * 1000 cm3/L
≈ 82 cm3
Therefore, approximately 82 cm3 of 1M HCl is necessary to dissolve 1g of magnesium ribbon.