iF 50.0 g of iron (II) carbonate react completely with hydrochloric acid, how many grams of carbon dioxide gas may be produced?
Here is a worked example of a stoichiometry problem. http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the number of grams of carbon dioxide gas produced when 50.0 g of iron (II) carbonate reacts completely with hydrochloric acid, you need to calculate the mole ratio between iron (II) carbonate and carbon dioxide.
Here's how you can do it:
1. Write the balanced chemical equation for the reaction:
FeCO3 + 2HCl -> FeCl2 + CO2 + H2O
2. Find the molar mass of iron (II) carbonate (FeCO3):
Fe: 55.9 g/mol
C: 12.0 g/mol
O: 16.0 g/mol
Molar mass of FeCO3:
55.9 + 12.0 + (16.0 * 3) = 115.9 g/mol
3. Convert the given mass of iron (II) carbonate (50.0 g) to moles:
moles = mass (g) / molar mass (g/mol)
moles = 50.0 g / 115.9 g/mol
4. Determine the mole ratio between FeCO3 and CO2 from the balanced chemical equation:
From the balanced equation, we can see that the ratio between FeCO3 and CO2 is 1:1.
5. Calculate the moles of CO2 produced:
Since the mole ratio between FeCO3 and CO2 is 1:1, the moles of CO2 produced will be the same as the moles of FeCO3.
6. Convert moles of CO2 to grams using the molar mass of CO2:
molar mass of CO2 = 12.0 + (16.0 * 2) = 44.0 g/mol
grams of CO2 = moles of CO2 * molar mass of CO2
By following these steps, you will be able to calculate the grams of carbon dioxide gas produced.