Respuesta :
Answer:
A. 182.3 grams of HCl, are consumed.
B. The reaction produce 5 g of H₂ and 238 g of MgCl₂
Explanation:
This the balanced equation:
Mg (s) + 2HCl (aq) → MgCl₂(aq) + H₂(g)
Ratio between Mg and HCl is 1:2, so if I react 2.5 moles of Mg, I use the double of moles, of Hydrochloridric (5 moles)
Molar mass of HCl = 36.46 g/m
Mass = Moles . Molar mass
Mass = 5 m . 36.46 g/m → 182.3 g
In this case, we have no limiting reactant and nothing is in excess. It is the same for the calculations to do the rule of three.
1 mol of Mg makes 1 mol of MgCl₂
2.5 moles of Mg makes 2.5 moles of MgCl₂
2 mol of HCl makes 1 mol of MgCl₂
5 moles of HCl makes 2.5 moles of MgCl₂
In conlussion, this reaction makes 2.5 moles of MgCl₂ and 2.5 moles of H₂
Molar mass H₂ = 2 g/m
Molar mass MgCl₂ = 95.2 g/m
2.5 moles . 2 g/m = 5 g H₂
2.5 moles . 95.2 g/m = 238 g MgCl₂
A. The mass of HCl is consumed is 182.3 grams.
B. The mass of each product is produced is 5 g of H₂ and 238 g of MgCl₂
Calculation of the mass:
A.
We know that
The balanced equation is
Mg (s) + 2HCl (aq) → MgCl₂(aq) + H₂(g)
The ratio between Mg and HCl should be 1:2.
Due to this if I react 2.5 moles of Mg, So here I use the double of moles, of Hydrochloridric (5 moles)
So,
Molar mass of HCl = 36.46 g/m
Now
Mass = Moles . Molar mass
Mass = 5 m . 36.46 g/m → 182.3 g
B.
We know that
1 mol of Mg makes 1 mol of MgCl₂
Likewise
2.5 moles of Mg makes 2.5 moles of MgCl₂
2 mol of HCl makes 1 mol of MgCl₂
5 moles of HCl makes 2.5 moles of MgCl₂
Now
Molar mass H₂ = 2 g/m
So,
Molar mass MgCl₂ = 95.2 g/m
Now
2.5 moles . 2 g/m = 5 g H₂
And,
2.5 moles . 95.2 g/m = 238 g MgCl₂
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