2HCl(aq) + Ca(s) → CaCl2(aq) + H2(g), Use the periodic table to find the atomic mass of Ca, Cl and H. If 80 grams of Ca react completely with HCl, what is the total mass of the products?

Answer 1

To find the total mass of the products formed from the reaction of calcium (Ca) with hydrochloric acid (HCl), we first need to determine the atomic masses of the elements involved in the reaction:

• Atomic mass of Calcium (Ca) ≈ 40.08 g/mol
• Atomic mass of Chlorine (Cl) ≈ 35.45 g/mol
• Atomic mass of Hydrogen (H) ≈ 1.01 g/mol

Now, let's calculate the molar mass of each compound formed in the reaction:

1. Molar mass of CaCl2:

   • Ca = 40.08 g/mol
   • Cl2 = 2 × 35.45 g/mol = 70.90 g/mol
   • Total molar mass of CaCl2 = 40.08 g/mol + 70.90 g/mol = 110.98 g/mol

2. Molar mass of H2:

   • H2 = 2 × 1.01 g/mol = 2.02 g/mol

Now, we can analyze the balanced chemical reaction: $$2\text{HCl(aq)}+\text{Ca(s)}\to {\text{CaCl}}_2\text{(aq)}+{\text{H}}_2\text{(g)}$$

From the balanced equation:

• 1 mole of Ca reacts with 2 moles of HCl to produce 1 mole of CaCl2 and 1 mole of H2.

Next, calculate the moles of Ca in 80 grams: $$\text{Moles of Ca}=\frac{\text{mass}}{\text{molar mass}}=\frac{80\text{ g}}{40.08\text{ g/mol}}\approx 1.99\text{ moles}$$

According to the balanced equation, 1 mole of Ca produces:

• 1 mole of CaCl2
• 1 mole of H2

Thus, 1.99 moles of Ca will produce 1.99 moles of CaCl2 and 1.99 moles of H2.

Now, let's calculate the mass of the products:

1. Mass of CaCl2 produced: $$\text{Mass of CaCl2}=\text{moles}\times \text{molar mass}=1.99\text{ moles}\times 110.98\text{ g/mol}\approx 220.59\text{ g}$$

2. Mass of H2 produced: $$\text{Mass of H2}=\text{moles}\times \text{molar mass}=1.99\text{ moles}\times 2.02\text{ g/mol}\approx 4.02\text{ g}$$

Total mass of the products: $$\text{Total mass}=\text{Mass of CaCl2}+\text{Mass of H2}\approx 220.59\text{ g}+4.02\text{ g}=224.61\text{ g}$$

Thus, the total mass of the products formed from the reaction is approximately 224.61 grams.