Question

if two solutions, one containing .2829 grams of cuso4 and the other one, 1.0742 grams kl are mixed and allowed to react, what mass in grams of i2 can be theoretically found in the reaction products ? use molar mass M(CuSO4) =159.609g/mol M(KL) =166.0028 g/mol, M(I2)=253.8089 g/moluse equation = 2CuSO4+4Kl -> 2Cul+I2+2K2SO4​

Answer 1

The maximum theoretical mass of I₂ that can be produced from the reaction of 0.2829 g of CuSO₄ and 1.0742 g of KI is 0.225 g.

Step-by-step explanation:

Given:

Molar mass of CuSO₄ (M(CuSO₄)) = 159.609 g/mol

Molar mass of KI (M(KI)) = 166.0028 g/mol

Molar mass of I₂ (M(I₂)) = 253.8089 g/mol

Reactant masses:

Mass of CuSO₄ (m(CuSO₄)) = 0.2829 g

Mass of KI (m(KI)) = 1.0742 g

Step 1: Calculate the moles of the reactants

Moles of CuSO₄ (n(CuSO₄)) = m(CuSO₄) / M(CuSO₄) = 0.2829 g / 159.609 g/mol ≈ 0.001777 mol

Moles of KI (n(KI)) = m(KI) / M(KI) = 1.0742 g / 166.0028 g/mol ≈ 0.006468 mol

Step 2: Determine the limiting reactant

Mole ratio = n(CuSO₄) / n(KI) ≈ 0.275

Since the mole ratio is less than 0.5, CuSO₄ is the limiting reactant.

Step 3: Calculate the theoretical yield of I₂

Based on the balanced chemical equation, 2 moles of CuSO₄ react to produce 1 mole of I₂.

Therefore, the theoretical yield of I₂ can be calculated as follows:

n(I₂) = (0.5) × n(CuSO₄) = (0.5) × 0.001777 mol ≈ 0.0008885 mol

Theoretical yield of I₂ (m(I₂)) = n(I₂) × M(I₂) = 0.0008885 mol × 253.8089 g/mol ≈ 0.2253 g

Step 4: Round the answer to the appropriate number of significant figures

The mass of CuSO₄ (0.2829 g) has 4 significant figures.

The mass of KI (1.0742 g) has 5 significant figures.

The molar masses of CuSO₄, KI, and I₂ have 4 significant figures each.

Therefore, the theoretical yield of I₂ should be rounded to 4 significant figures:

Theoretical yield of I₂ (m(I₂)) ≈ 0.2253 g ≈ 0.225 g