In Atomic Radiusthe more protons there are the A.smaller the electrons
B. Weaker the pull
C.stronger the pull
D.bigger the electrons

A. HCl is the limiting reactant.

B. Theoretical yield of Cl₂ is 20.9 g.

C. Actual yield of Cl₂ = 15.2 g.

Explanation:

The balanced equation for the reaction is given below:

4HCl + MnO₂ –> MnCl₂ + 2H₂O + Cl₂

Next, we shall determine the masses of HCl and MnO₂ that reacted and the mass of Cl₂ produced from the balanced equation. This can be obtained as follow:

Molar mass of HCl = 1 + 35.5

= 36.5 g/mol

Mass of HCl from the balanced equation = 4 × 36.5 = 146 g

Molar mass of MnO₂ = 55 + (2×16)

= 55 + 32

= 87 g/mol

Mass of MnO₂ from the balanced equation = 1 × 87 = 87 g

Molar mass of Cl₂ = 2 × 35.5

= 71 g/mol

Mass of Cl₂ from the balanced equation = 1 × 71 = 71 g

SUMMARY:

From the balanced equation above,

146 g of HCl reacted with 87 g of MnO₂ to produce 71 g of Cl₂.

A. Determination of the limiting reactant.

From the balanced equation above,

146 g of HCl reacted with 87 g of MnO₂.

Therefore, 42.9 g of HCl will react with = (42.9 × 87)/146 = 25.6 g of MnO₂.

From the calculation made above, we can see clearly that only 25.6 g out of 43.1 g of MnO₂ given was needed to react completely with 42.9 g of HCl.

Therefore, HCl is the limiting reactant.

B. Determination of theoretical yield of Cl₂.

Here, the limiting reactant will be used.

From the balanced equation above,

146 g of HCl reacted to produce 71 g of Cl₂.

Therefore, 42.9 g of HCl will react to produce = (42.9 × 71)/146 = 20.9 g of Cl₂.

Thus, the theoretical yield of Cl₂ is 20.9 g.

C. Determination of the actual yield of Cl₂.

Theoretical yield of Cl₂ = 20.9 g

Percentage yield of Cl₂ = 72.9%

Actual yield of Cl₂ =?

Percentage yield = Actual yield / Theoretical yield × 100

72.9% = Actual yield / 20.9

Cross multiply

Actual yield = 72.9% × 20.9

Actual yield = 72.9/100 × 20.9

Actual yield = 0.729 × 20.9

Actual yield of Cl₂ = 15.2 g