The antacid in question (with an active ingredient of Ca(HCO3)2), upon treatment with excess hydrochloric acid, a 0.413 g sample gives 92.85 mL of CO2 at 25.00oC and 1.000 atm. What percentage of the antacid is active ingredient? Assume a perfect system (i.e. the yield is 100%)

Ca(HCO3)2 + 2HCl ==> CaCl2 + 2H2O + 2CO2

Use PV = nRT. Substitute and solve for n.
mols x molar mass = grams CO2.
Convert g CO2 to g Ca(HCO3)2
(g Ca(HCO3)2/mass sample)*100 = % Ca(HCO3)2

dont you have to convert mols CO2 to mols Ca(HCO3)2 first?

dont you have to convert mols CO2 to mols Ca(HCO3)2 first? then convert to get grams?

To find the percentage of the antacid that is the active ingredient (Ca(HCO3)2), we need to determine the amount of CO2 produced from the reaction and then use stoichiometry to convert it to the amount of Ca(HCO3)2.

Step 1: Calculate moles of CO2 produced
We need to calculate the moles of CO2 produced based on the given volume, temperature, and pressure. We can use the ideal gas law equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, convert the given temperature of 25.00oC to Kelvin by adding 273.15:
T = 25.00oC + 273.15 = 298.15 K

Now, substitute the values into the ideal gas law equation:
1.000 atm * 0.09285 L = n * 0.0821 L*atm/(mol*K) * 298.15 K

Solving for n, we get:
n = (1.000 atm * 0.09285 L) / (0.0821 L*atm/(mol*K) * 298.15 K)

Step 2: Calculate moles of Ca(HCO3)2
The balanced chemical equation for the reaction between Ca(HCO3)2 and HCl is:
Ca(HCO3)2 + 2HCl -> CaCl2 + 2CO2 + 2H2O

The stoichiometric ratio between Ca(HCO3)2 and CO2 is 1:2. This means that for every 1 mole of Ca(HCO3)2, 2 moles of CO2 are produced.

Since we have calculated the moles of CO2 in Step 1, we can use the stoichiometric ratio to determine the moles of Ca(HCO3)2. Multiply the moles of CO2 by the mole ratio:
moles of Ca(HCO3)2 = moles of CO2 * (1 mole Ca(HCO3)2 / 2 moles CO2)

Step 3: Calculate the mass percentage of active ingredient
The required mass percentage of the active ingredient is the mass of the active ingredient divided by the mass of the sample, multiplied by 100.

Given that the mass of the sample is 0.413 g, and we have calculated the moles of Ca(HCO3)2, we can calculate the mass of the active ingredient (Ca(HCO3)2) using its molar mass (which is 162.11 g/mol):

mass of active ingredient = moles of Ca(HCO3)2 * molar mass of Ca(HCO3)2

Finally, we can calculate the mass percentage:
mass percentage = (mass of active ingredient / mass of the sample) * 100

By following these steps, you should be able to find the percentage of the antacid that is the active ingredient (Ca(HCO3)2).