When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of 9.0 M HCl is required to react completely with 5.00 g of magnesium?
Mg + 2HCl ==> H2 + MgCl2
Convert 5.00 g Mg to moles. moles = grams/molar mass
Using the coefficients in the balanced equation, convert moles Mg to moles HCl.
You know moles HCl = M x L.
You moles and M, solve for L.
To solve this problem, we need to use the balanced chemical equation for the reaction between hydrochloric acid (HCl) and magnesium (Mg):
2 HCl + Mg -> MgCl2 + H2
From the equation, we can see that 2 moles of HCl react with 1 mole of Mg to produce 1 mole of MgCl2 and 1 mole of H2.
Step 1: Calculate the number of moles of magnesium (Mg):
To calculate the number of moles of Mg, we need to use its molar mass, which is 24.31 g/mol.
Moles of Mg = mass / molar mass
Moles of Mg = 5.00 g / 24.31 g/mol
Moles of Mg = 0.206 moles
Step 2: Use the balanced equation to calculate the number of moles of HCl required:
According to the balanced equation, 2 moles of HCl react with 1 mole of Mg.
Moles of HCl = (0.206 moles Mg) / (1 mole Mg) * (2 moles HCl) / (1 mole Mg)
Moles of HCl = 0.412 moles
Step 3: Calculate the volume of 9.0 M HCl required:
The molarity of HCl is given as 9.0 M, which means there are 9.0 moles of HCl in 1 liter (1000 mL) of the solution.
Volume of HCl = Moles of HCl / Molarity of HCl
Volume of HCl = 0.412 moles / 9.0 M
Volume of HCl = 0.0458 L or 45.8 mL
Therefore, you would require 45.8 mL of 9.0 M HCl to react completely with 5.00 g of magnesium.
To determine the volume of 9.0 M hydrochloric acid (HCl) required to react completely with 5.00 g of magnesium (Mg), you need to use the balanced chemical equation and stoichiometry.
1. Write the balanced chemical equation:
Mg + 2HCl -> MgCl2 + H2
2. Determine the molar mass of magnesium:
Mg = 24.31 g/mol
3. Use the molar mass to convert the mass of magnesium to moles:
moles of Mg = mass of Mg / molar mass of Mg
moles of Mg = 5.00 g / 24.31 g/mol
4. Apply stoichiometry to find the moles of HCl required:
From the balanced equation, we see that 1 mole of magnesium reacts with 2 moles of HCl.
moles of HCl = 2 * moles of Mg
5. Calculate the volume of 9.0 M HCl using the molarity formula:
Molarity = moles of solute / volume of solution (in Liters)
volume of HCl (in Liters) = moles of HCl / Molarity of HCl
Now we can plug in the values:
moles of HCl = 2 * (5.00 g / 24.31 g/mol)
= 0.411 mole (rounded to 3 decimal places)
volume of HCl (in Liters) = 0.411 mol / 9.0 mol/L
= 0.046 L (rounded to 3 decimal places)
To convert the volume to milliliters (mL), multiply by 1000:
volume of HCl = 0.046 L * 1000 mL/L
= 46 mL
Therefore, approximately 46 mL of 9.0 M HCl is required to react completely with 5.00 g of magnesium.