20 grams of solid calcium carbonate is placed in a flaks with excess hydrochloric...?

Question

20 grams of solid calcium carbonate is placed in a flask with excess hydrochloric acid at 30 C. what volume of dry CO2 will be produced?

plz answer quick becuz i have to know how to do this when the test comes up.

Answer 1

CaCO3 & 2 HCl --> CO2 & H2O & CaCl2

the equation shows that  one mole of CaCO3 ( mass = 100.0 g/mol) produces 1 mole of CO2, so let's find the moles of CO2 produced:

20 grams CaCO3 @ 100g/mole = 0.20 moles of CaCO3

0.20 moles of CaCO3  =  0.20 moles of CO2

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now ,you will have to know the barometric pressure that the gas was collected at,

and  if the gas was not dried, you will have to subtract the vapor pressure of water @ 30 C (31.8 torr) to get the pressure of CO2 collected.

I am going to assume that the barometric pressure is 760Torr, and that is was collected over water & not run through a drying chamber.

therfore 760 - 31.8 = 728 Torr of CO2 was generated

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now your question:

PV=nRT

(728T)(V) = 0.20 moles (62.36 Torr-litres / mol-K)(303K)

V = 5.17 litres

that could be your answer, but it depends upon the significant digits in "20 grams" which only has 1 sig fig

your answer(1sigfig in 20 grams): 5 litres of CO2 produced

your answer(2igfig in 20.grams): 5.2 litres of CO2 produced

your answer(3sigfig in 20.0 grams): 5.17 litres CO2 produced