Asked by nichole
How many liters of CO2 form at STP if 5.0g of CaCO3 are treated with excess hydrochloric acid? show all your work
Answers
Answered by
DrBob222
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.
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.
Answered by
Anonymous
3+5=8
Answered by
taylor
1.12 liters
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