Question

If 47.2 g of calcium chloride reacts with 135.2 g of nickel arsenate according to the following balanced equation, how many grams of nickel chloride are produced? 3 CaCl2 + Ni3(AsO₄)2 → 3 NiCl2 + Ca₃⁺(AsO₄)2

Answer 1

To find the grams of nickel chloride produced in a chemical reaction between calcium chloride and nickel arsenate, convert the given masses to moles, use the stoichiometric ratio to determine the moles of nickel chloride, and then convert back to grams.

Step-by-step explanation:

To find the number of grams of nickel chloride (NiCl2) produced, we need to use the given quantities and the stoichiometry of the balanced equation. First, we convert the given masses of calcium chloride (CaCl2) and nickel arsenate (Ni3(AsO4)2) to moles by dividing by their respective molar masses. We then use the stoichiometric ratio of the reactants and products to determine the number of moles of nickel chloride produced. Finally, we convert the moles of nickel chloride back to grams by multiplying by its molar mass.

Given:

• Mass of CaCl2 = 47.2 g
• Mass of Ni3(AsO4)2 = 135.2 g

Step 1: Convert masses to moles:

• Moles of CaCl2 = 47.2 g / molar mass of CaCl2
• Moles of Ni3(AsO4)2 = 135.2 g / molar mass of Ni3(AsO4)2

Step 2: Determine moles of nickel chloride produced:

• According to the stoichiometry of the balanced equation, the molar ratio of CaCl2 to NiCl2 is 3:3. Therefore, moles of NiCl2 = moles of CaCl2

Step 3: Convert moles of nickel chloride to grams:

• Mass of NiCl2 = moles of NiCl2 * molar mass of NiCl2

Substituting the given values and performing the calculations will give you the mass of nickel chloride produced.