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.
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?
2 answers
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.