73.0 WHAT</b) of carbon dioxide?????
I will assume you mean grams but if not grams you must adjust the work accordingly.
You have the balanced equation.
2. Convert 73.0 g CO2 to mols. moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles CO2 to moles CaCO3.
4. Now convert moles CaCO3 to grams. grams CaCO3 = moles CaCO3 x molar mass CaCO3.
When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction
CaCO3 ---> CaO + CO2
How many grams of calcium carbonate are needed to produce 73.0 of carbon dioxide at STP?
7 answers
73 g CO2 is how many moles?
From the balanced equation, it takes one mole of calcium carbonate to produced one mole of carbon dioxide.
From the balanced equation, it takes one mole of calcium carbonate to produced one mole of carbon dioxide.
I did it like
76.0Lof CO2/22.4L = 3.2589moles of CO2
Moles of CO2 = Moles of CaCaCO3
to convert it in g's:
3.2589moles of CaCO3*(100g/1mole Of CaCO3)
= 325.89g
76.0Lof CO2/22.4L = 3.2589moles of CO2
Moles of CO2 = Moles of CaCaCO3
to convert it in g's:
3.2589moles of CaCO3*(100g/1mole Of CaCO3)
= 325.89g
OK. So it's 73.0 LITERS. You made a typo in your work where you typed 76.0 BUT your answer is correct for 73.0/22.4. If you are keying this answer into an on-line database, I suspect your answer is coming back wrong because you are posting too many significant figures. Your answer should be rounded to 326 grams CaCO3.
ohh yea i figured that out. nd thnxxx a lot fohh ur help.
130.28 gr
166 gr
2 answers