In the lab, students decomposed a sample of calcium carbonate by heating it over a Bunsen burner and collected carbon dioxide according to the following equation:
CaCO3(s) --- > CaO(s) + CO2(g)
(a) How many mL of carbon dioxide gas were generated by the decomposition of 5.83 g of calcium carbonate at STP
(b) How many moles of calcium carbonate would be required to generate 67.6 L of carbon dioxide at STP?
a. mols CaCO3 = grams/molar mass == 5.83/100 = 0.583.
According to the equation, 1 mol of CO2 is generated for every 1 mol CaCO3; therefore, we can expect 0.583 mols CO2 @ STP.
Then you know 1 mol of a gas occupies 22.4 L @ STP so 0.583 mols will occupy 0.583 mols x 22.4 L/mol = ? L. Convert that to mL.
b. This is backwards of part a. Post your work if you get stuck.
In the future you should show SOME work and/or tell us specifically what you don't understand about the process. This is not a homework dump site where you go to a movie with a date while we do your homework for you.
this is exactly a homework dump its only used to cheat while other students use it for "checking their answers" while they just actually use it to cheat since they dont wanna put the time and effort in and believe they think school is useless and believe to just merry a rich person. yes this generation not. good.
To solve these questions, we need to use the concept of stoichiometry. Stoichiometry allows us to relate the amounts of reactants and products in a chemical reaction. Here's how you can solve each question:
(a) To find the volume of carbon dioxide generated, we need to know the molar volume of gas at STP. The molar volume of any ideal gas at STP is 22.4 L/mol.
Step 1: Calculate the number of moles of calcium carbonate (CaCO3).
Given: Mass of CaCO3 = 5.83 g
Molar mass of CaCO3 = 40.08 g/mol + 12.01 g/mol + 3 * 16.00 g/mol = 100.09 g/mol
Number of moles of CaCO3 = Mass of CaCO3 / Molar mass of CaCO3
Number of moles of CaCO3 = 5.83 g / 100.09 g/mol
Step 2: Use stoichiometry to relate the number of moles of CaCO3 to the number of moles of CO2.
From the balanced equation: 1 mole of CaCO3 produces 1 mole of CO2.
Number of moles of CO2 = Number of moles of CaCO3
Step 3: Convert moles of CO2 to volume (in mL) at STP.
Volume of CO2 (in L) = Number of moles of CO2 * Molar volume of gas at STP
Volume of CO2 (in L) = Number of moles of CO2 * 22.4 L/mol
Volume of CO2 (in mL) = Volume of CO2 (in L) * 1000 mL/L
(b) To find the number of moles of calcium carbonate needed to generate 67.6 L of carbon dioxide at STP, we will again use stoichiometry.
Step 1: Determine the number of moles of CO2 using the same formula as in part (a).
Number of moles of CO2 = Volume of CO2 (in L) / Molar volume of gas at STP
Step 2: Use stoichiometry to relate the number of moles of CO2 to the number of moles of CaCO3.
From the balanced equation, 1 mole of CaCO3 produces 1 mole of CO2.
Number of moles of CaCO3 = Number of moles of CO2
That's how you can solve these questions using stoichiometry.