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- Homework Statement:
- Thermal decomposition of calcium hydrogen carbonate yields calcium carbonate water and carbon dioxide. Calculate the volume of carbon dioxide measured at 0 °C and 1.00 atm that is obtained by heating 80.0 grams of calcium carbonate

- Relevant Equations:
- gas laws

Ca(HCO

First I evaluate the moles of calcium carbonate (don't mind the units, just to save time)

##\frac {80.0}{40,00+12.01+3*16,00}= 0,799 mol##

From the equation, correct me if I am wrong , one mole of CaCO

Using the ideal gas law equation PV=nRT, I can compute V:

##V=\frac{nRT}{P} ##

inserting the values, I don't get the expected result, so I suspect that something is wrong, Any help ?

_{3})2 -> CaCO_{3}+ H_{2}O + CO_{2}First I evaluate the moles of calcium carbonate (don't mind the units, just to save time)

##\frac {80.0}{40,00+12.01+3*16,00}= 0,799 mol##

From the equation, correct me if I am wrong , one mole of CaCO

_{3}is proportional to one mole of CO_{2}, so from this I can say that also CO_{2}has 0,799 mol.Using the ideal gas law equation PV=nRT, I can compute V:

##V=\frac{nRT}{P} ##

inserting the values, I don't get the expected result, so I suspect that something is wrong, Any help ?