calculate the number of moles of magnesium chloride produced by reacting 168g of magnesium trioxocarbonate(iv)with excess hydrochloric acid(mg=24,c=12,o=16,h=1,cl=35.5)
write the balanced equation
how many moles in 168 grams?
The equation will tell you how many moles of MgCl2 to expect
To calculate the number of moles of magnesium chloride produced, we need to follow these steps:
Step 1: Calculate the molar mass of magnesium trioxocarbonate(IV)
Molar mass of magnesium(Mg) = 24 g/mol
Molar mass of carbon(C) = 12 g/mol
Molar mass of oxygen(O) = 16 g/mol
Molar mass of magnesium trioxocarbonate(IV) = (Mg + 3O + C) = (24 + 3(16) + 12) g/mol = 84 g/mol
Step 2: Convert mass (in grams) of magnesium trioxocarbonate(IV) to moles
Mass of magnesium trioxocarbonate(IV) = 168 g
Moles of magnesium trioxocarbonate(IV) = mass / molar mass
Moles of magnesium trioxocarbonate(IV) = 168 g / 84 g/mol
Moles of magnesium trioxocarbonate(IV) = 2 mol
Step 3: Determine the stoichiometry of the reaction
The balanced chemical equation for the reaction between magnesium trioxocarbonate(IV) and hydrochloric acid is:
MgCO3 + 2HCl -> MgCl2 + H2O + CO2
This means that for every 1 mole of magnesium trioxocarbonate(IV) reacted, 1 mole of magnesium chloride is produced.
Step 4: Calculate the number of moles of magnesium chloride produced
Number of moles of magnesium chloride = Number of moles of magnesium trioxocarbonate(IV)
Number of moles of magnesium chloride = 2 mol
Therefore, 2 moles of magnesium chloride are produced by reacting 168g of magnesium trioxocarbonate(IV) with excess hydrochloric acid.
To calculate the number of moles of magnesium chloride produced, we need to follow these steps:
1. Determine the balanced chemical equation for the reaction between magnesium trioxocarbonate(IV) (also known as magnesium carbonate) and hydrochloric acid:
MgCO3 + 2HCl → MgCl2 + H2O + CO2
2. Find the molar mass of magnesium trioxocarbonate(IV) (MgCO3) and magnesium chloride (MgCl2):
- The molar mass of MgCO3 = (1 × Mg) + (1 × C) + (3 × O) = 24 + 12 + (3 × 16) = 84 g/mol
- The molar mass of MgCl2 = (1 × Mg) + (2 × Cl) = 24 + (2 × 35.5) = 95 g/mol
3. Convert the given mass of MgCO3 (168 g) into moles:
- Moles = Mass / Molar mass
- Moles of MgCO3 = 168 g / 84 g/mol = 2 moles
4. Use the stoichiometry of the balanced equation to determine the number of moles of MgCl2 produced, considering that the reaction is taking place with an excess of hydrochloric acid. From the balanced equation, we can see that:
1 mole of MgCO3 reacts to produce 1 mole of MgCl2
Therefore, 2 moles of MgCO3 will produce 2 moles of MgCl2.
So, when 168 g of magnesium trioxocarbonate(IV) reacts, it will produce 2 moles of magnesium chloride.