How many liters of CO2 form at STP if 5.0g of CaCO3 are treated with excess hydrochloric acid? show all your work

Answer 1

Write the equation and balance it.
Convert 5.0 g CaCO3 to moles. Moles = grams/molar mass.
Using the coefficients in the balanced equation, convert moles CaCO3 to moles CO2.
Convert moles CO2 to volume (since this is at STP you know that 1 mole CO2 at STP will occupy 22.4 L). So moles from the previous step x 22.4 L/mole = liters CO2.
Post your work if you get stuck.

Answer 2

3+5=8

Answer 3

1.12 liters