Marble (calcium carbonate) reacts with hydrochloric acid solution to form calcium

chloride solution, water and carbon dioxide. What is the percent yield of carbon dioxide
if 3.65 g of the gas is collected when 10.0 g marble reacts?

CaCO3 + 2 HCl → CaCl2 + CO2 + H2O

10.0 g CaCO3 is .1 mole ... so .1 mole of CO2 should be produced

molar mass CO2 ... 44.0 g

% yield ... (3.65 / 4.40) * 100%

Well, it seems like marble got a little excited and released some gas during the reaction. Good for it! Now let's calculate the percent yield of carbon dioxide.

To start, we need to determine the theoretical yield of carbon dioxide. We know that for every mole of marble (CaCO3), one mole of carbon dioxide (CO2) is produced. So, let's calculate the moles of marble:

Molar mass of CaCO3 = 40.08 g/mol + 12.01 g/mol + (3 x 16.00 g/mol) = 100.09 g/mol

Moles of marble = 10.0 g / 100.09 g/mol = 0.0999 mol (let's keep it rounded to 0.1 mol for simplicity).

Since the mole ratio between marble and carbon dioxide is 1:1, the moles of carbon dioxide produced will also be 0.1 mol.

Now let's calculate the actual yield of carbon dioxide, which is given as 3.65 g.

Percent yield = (Actual yield / Theoretical yield) x 100
Percent yield = (3.65 g / (0.1 mol x 44.01 g/mol)) x 100
Percent yield = (3.65 g / 4.401 g) x 100
Percent yield ≈ 82.89%

So, the percent yield of carbon dioxide is approximately 82.89%. Marble did a pretty good job, didn't it? I hope all this chemistry didn't leave you feeling...marbelous!

To calculate the percent yield of carbon dioxide, we need to compare the actual yield (3.65 g) to the theoretical yield.

First, let's calculate the moles of carbon dioxide produced by the reaction:

1 mol of CaCO3 reacts with 1 mol of CO2.
The molar mass of CaCO3 is 100.09 g/mol.

Step 1: Calculate moles of CaCO3:
moles of CaCO3 = mass of CaCO3 / molar mass of CaCO3
moles of CaCO3 = 10.0 g / 100.09 g/mol
moles of CaCO3 = 0.0999 mol

Step 2: Calculate moles of CO2 (theoretical yield):
moles of CO2 = moles of CaCO3
moles of CO2 = 0.0999 mol

Step 3: Calculate the theoretical yield of CO2 in grams:
mass of CO2 (theoretical yield) = moles of CO2 × molar mass of CO2
mass of CO2 (theoretical yield) = 0.0999 mol × 44.01 g/mol
mass of CO2 (theoretical yield) = 4.40 g

Now, we can calculate the percent yield:

percent yield = (actual yield / theoretical yield) × 100%
percent yield = (3.65 g / 4.40 g) × 100%
percent yield = 0.8295 × 100%
percent yield = 82.95%

Therefore, the percent yield of carbon dioxide in this reaction is approximately 82.95%.

To find the percent yield of carbon dioxide, we need to compare the amount of carbon dioxide produced to the theoretical yield of carbon dioxide.

First, we need to calculate the theoretical yield of carbon dioxide. We can do this by using the balanced chemical equation of the reaction:

CaCO3 + 2HCl -> CaCl2 + H2O + CO2

From the equation, we can see that 1 mole of CaCO3 reacts to produce 1 mole of CO2. We can find the number of moles of CaCO3 by dividing the mass of the marble by its molar mass:

Molar mass of CaCO3 = (40.08 g/mol of Ca) + (12.01 g/mol of C) + (3 x 16.00 g/mol of O) = 100.09 g/mol
Number of moles of CaCO3 = mass of marble / molar mass of CaCO3 = 10.0 g / 100.09 g/mol = 0.09991 mol

Since the mole ratio between CaCO3 and CO2 is 1:1, the moles of CO2 produced will also be 0.09991 mol.

Now, to find the percent yield of CO2, we divide the actual yield (3.65 g) by the theoretical yield (calculated above) and multiply by 100:

Percent yield = (actual yield / theoretical yield) x 100
Percent yield = (3.65 g / 0.09991 mol) x 100 = 365.45%

Therefore, the percent yield of carbon dioxide in this reaction is 365.45%.