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    phylicia's Avatar
    phylicia Posts: 1, Reputation: 1
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    #1

    Sep 20, 2009, 11:37 AM
    Chemistry Trouble
    CaCO3+2HCl=CaCl2+CO2+H2O.How many grams of CO2 are formed by complete reaction with 33.7 of limestone? What is the volume of CO2 at STP?
    marzipan6's Avatar
    marzipan6 Posts: 9, Reputation: 3
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    #2

    Sep 20, 2009, 06:28 PM

    If you've done any practice questions or examples in class, go back and check these out. I don't really know what grade you are in or what kind of chemistry training you've had, so I don't want to give you an answer that is over your head, but you do need to use molar mass, which is the addition of atomic masses of all the elements in a molecule, mole ratios, and the formula n=m/M, where n is the number of moles, m is mass in grams, and M is the molar mass in grams. As for the volume, I was taught that 1 mole of gas at STP is 22.4 litres, which comes from the formula PV=nRT, where P is pressure (1atm at STP), V is volume in litres, n is the number of moles, R is the constant 0.08206 atmxmolxK, and T is temp in Kelvins (273 at STP).
    Perito's Avatar
    Perito Posts: 3,139, Reputation: 150
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    #3

    Sep 20, 2009, 08:24 PM
    Quote Originally Posted by phylicia View Post

    CaCO3+2HCl=CaCl2+CO2+H2O.How many grams of CO2 are formed by complete reaction with 33.7 of limestone? What is the volume of CO2 at STP?
    If you assume that CO2 is an ideal gas, one mole of any ideal gas will occupy 22.4 liters. You can find that from the ideal gas law, PV=nRT.

    Limestone is CaCO3. Figure out how many moles of CaCO3 you have. Then using the balanced equation, figure out how many moles of CO2 will be produced. You can then use the ideal gas law to figure out the volume.

    STP = 0 Celsius and 1 atmosphere.
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