Question

If 4.50 g of HCl are reacted with 15.00 g of Caco, according to the following balanced chemical equation, calculate the theoretical yield of.CO. 2HCl + CaCO3 CaCl2 + H2O + CO2 if 2.50 g of CO2 are isolated, after carrying out the above reaction, calculate the percent yield of CO2.

Answer 1

Answer: HCl is the limiting reactant and the theoretical yield is 2.72 g of CO2. If the actual yield was 2.50 g then, the percent yield is 92.0% when rounding off is done only for the final answer.  

Further Explanation:

In order to determine the theoretical yield and the percent yield of CO2, the following steps must be done:

1. Determine the limiting reactant. This is the reactant that will determine the amount of CO2 that will actually form.
2. Determine the theoretical yield for CO2 when the limiting reactant is used.
3. Get the percent yield by getting the ratio of the actual yield stated in the problem and the calculated theoretical yield multiplied by 100.

Determining the Limiting Reactant

The Limiting Reactant (LR) will produce fewer moles of the products. To check  which of the reactants HCl or CaCO3 is the LR, we do dimensional analysis:

For HCl:

$moles\ CO_{2}\ = (4.50\ g\ HCl)\(\frac{1\ mol\ HCl}{36.46094\ g})( \frac{1\ mol\ CO_{2} }{2\ mol\ HCl}) \\moles\ CO_{2}\ =\ 0.0617098$

For CaCO3:

$moles\ of\ CO_{2}\ = (15.00\ g\ CaCO_{3})\ (\frac{1\ mol\ CaCO_{3} }{100.0869\ g\ CaCO_{3} })\ (\frac{1\ mol\ CO_{2} }{1\ mol\ CaCO_{3} })\\moles\ of\ CO_{2}\ = \ 0.1499$

Since HCl produces fewer moles of CO2, then it is the limiting reactant. We will use the given amount to determine the theoretical yield for CO2.

Determining the Theoretical Yield

From Step 1, we know that 0.0617098 moles of CO2 will be produced. We will just convert this to grams.

$grams\ CO_{2}\ =\ (0.0617098\ mol\ CO_{2})  (\frac{44.01\ g\ CO_{2}}{1\ mol\ CO_{2}})\\grams\ CO_{2}\ =\ 2.71585$

Since the answer only requires 3 significant figures, the final answer is 2.72 grams CO2.

Determining the Percent Yield

Dividing the actual yield by the theoretical yield will give us the percent yield, which is an indicator of how efficient the experiment or the method used was.

From the problem, the actual yield was 2.50 g, hence, the percent yield is:

$percent\ yield\ of\ CO_{2}\ = (\frac{2.50\ g}{2.71585\ g}) (100)\\percent\ yield\ of\ CO_{2}\ = 92.05221$

Rounding off to three significant figures, the percent yield is 92.0%. This suggests that the method used is somewhat efficient in producing CO2.

Learn More

1. Learn More about Limiting Reactant https://brainly.com/question/7144022
2. Learn More about Excess Reactant https://brainly.com/question/6091457  
3. Learn More about Stoichiometry https://brainly.com/question/9743981

Keywords: stoichiometry, theoretical yield, actual yield

Answer 2

1. The theoretical yield of CO₂ is 2.71 g

2. The percentage yield of CO₂ is 92.3%

We'll begin by calculating the masses of HCl and CaCO₃ that reacted and the mass of CO₂ produced from the balanced equation.

2HCl + CaCO₃ —> CaCl₂ + H₂O + CO₂

Molar mass of HCl = 1 + 35.5 = 36.5 g/mol

Mass of HCl from the balanced equation = 2 × 36.5 = 73 g

Molar mass of CaCO₃ = 40 + 12 + (3 × 16) = 100 g/mol

Mass of CaCO₃ from the balanced equation = 1 × 100 = 100 g

Molar mass of CO₂ = 12 + (2 × 16) = 44 g/mol

Mass of CO₂ from the balanced equation = 1 × 44 = 44 g

SUMMARY

From the balanced equation above,

73 g of HCl reacted with 100 g of CaCO₃ to produce 44 g of CO₂

• Next, we shall determine the limiting reactant.

From the balanced equation above,

73 g of HCl reacted with 100 g of CaCO₃

Therefore,

4.5 g of HCl will react with = (4.5 × 100)/73 = 6.16 g of CaCO₃

From the calculation made above, we can see that only 6.16 g of CaCO₃ out of 15 g given, reacted completely with 4.5 g of HCl.

Therefore, HCl is the limiting reactant and CaCO₃ is the excess reactant.

1. Determination of the theoretical yield of CO₂

From the balanced equation above,

73 g of HCl reacted to produce 44 g of CO₂

Therefore,

4.5 g of HCl will react to produce = (4.5 × 44)/73 = 2.71 g of CO₂

Thus, the theoretical yield of CO₂ is 2.71 g

2.. Determination of the percentage yield of CO₂

Actual yield of CO₂ = 2.50 g

Theoretical yield of CO₂ = 2.71 g

Percentage yield of CO₂ =?

$percentage \: = \frac{actual}{theoretical} \times 100 \\ \\ = \frac{2.5}{2.71} \times 100$

Percentage yield of CO₂ = 92.3%

Learn more: https://brainly.com/question/25669079