How do it geth the equation for 50.0 grams of iron(II)carbonate react completely with hydrochloric acid how many grams of carbon dioxide gas may be produced?
Robin, always start with the balanced equation.
FeCO3+ 2HCl>>CO2 + H2O+ FeCl2
So for each mole of iron(II) carbonate, one gets one mole of CO2.
So the issue is how many moles of FeCO3 do you have?
I assume you can take it from here.
To determine how many grams of carbon dioxide gas may be produced when 50.0 grams of iron(II) carbonate react completely with hydrochloric acid, you need to follow these steps:
1. Write a balanced chemical equation: First, write a balanced chemical equation for the reaction between iron(II) carbonate (FeCO3) and hydrochloric acid (HCl). The reaction equation is as follows:
FeCO3 + 2HCl → FeCl2 + CO2 + H2O
2. Calculate the molar mass: Find the molar mass of FeCO3 and CO2. The molar mass of FeCO3 is calculated by adding the atomic masses of the elements:
Fe (55.85 g/mol) + C (12.01 g/mol) + 3O (16.00 g/mol) = 115.86 g/mol
The molar mass of CO2 is calculated similarly:
C (12.01 g/mol) + 2O (16.00 g/mol) = 44.01 g/mol
3. Convert grams to moles: Use the molar mass to convert 50.0 grams of FeCO3 to moles.
Moles of FeCO3 = mass (g) / molar mass (g/mol)
Moles of FeCO3 = 50.0 g / 115.86 g/mol
4. Use stoichiometry: Since the balanced equation tells us that 1 mole of FeCO3 reacts to produce 1 mole of CO2, we can calculate the moles of CO2 produced.
Moles of CO2 = Moles of FeCO3
5. Convert moles to grams: Finally, convert moles of CO2 to grams using the molar mass of CO2.
Mass of CO2 = Moles of CO2 × molar mass of CO2
Mass of CO2 = Moles of CO2 × 44.01 g/mol
By following these steps, you will be able to calculate the mass of carbon dioxide gas that may be produced when 50.0 grams of iron(II)carbonate react completely with hydrochloric acid.