in a blast furnace, Iron(III) oxide is used to produce iron by the following unbalanced reaction....Fe2O3(s) + CO(g)-->Fe(s)+ CO2(g)
if 4.00 kg Fe2O3 are available to react how many moles of CO are needed? how many moles of each product are formed?
help please how do i balance this?
To balance the chemical equation, we need to ensure that the number of atoms of each element is equal on both sides. Here's a step-by-step guide on how to balance the equation:
1. Write down the unbalanced equation:
Fe2O3(s) + CO(g) → Fe(s) + CO2(g)
2. Count the number of atoms of each element on both sides of the equation:
Fe2O3(s): 2 Fe atoms, 3 O atoms
CO(g): 1 C atom, 1 O atom
Fe(s): 1 Fe atom
CO2(g): 1 C atom, 2 O atoms
3. Start balancing the equation by adjusting the coefficient in front of each compound. To do this, begin with the most complex compounds and elements that appear in only one location:
Fe2O3(s) + CO(g) → 2 Fe(s) + CO2(g)
Now, let's solve the given problems using the balanced equation:
1. To determine the number of moles of CO required to react with 4.00 kg of Fe2O3, we need to use the molar mass and stoichiometry of the balanced equation.
The molar mass of Fe2O3 is:
Fe: 55.85 g/mol x 2 = 111.7 g/mol
O: 16 g/mol x 3 = 48 g/mol
Total molar mass = 111.7 g/mol + 48 g/mol = 159.7 g/mol
To convert the mass of Fe2O3 to moles, we use the formula: Moles = Mass / Molar mass.
Moles of Fe2O3 = 4000 g / 159.7 g/mol = 25.06 mol
From the balanced equation: Fe2O3(s) + CO(g) → 2 Fe(s) + CO2(g), we can determine the stoichiometric ratio between Fe2O3 and CO.
For every 1 mol of Fe2O3, we need 1 mol of CO. Therefore, the moles of CO needed is also 25.06 mol.
2. The balanced equation tells us that 1 mol of Fe2O3 produces 2 mol of Fe and 1 mol of CO2.
Using the stoichiometric ratio, we know that:
25.06 mol of Fe2O3 produces 2 x 25.06 = 50.12 mol of Fe
25.06 mol of Fe2O3 produces 25.06 mol of CO2
Therefore, the number of moles of each product formed is:
Moles of Fe = 50.12 mol
Moles of CO2 = 25.06 mol
Remember to always balance chemical equations to ensure accurate calculations and understanding of reactants and products.
To balance the equation, follow these steps:
Step 1: Make a table listing the number of atoms for each element on both sides of the equation.
Element | Fe2O3 | CO | Fe | CO2
---------------------------------------
Iron (Fe) | 2 | 0 | 1 | 0
Carbon (C) | 0 | 1 | 0 | 1
Oxygen (O) | 3 | 0 | 0 | 2
Step 2: Balance each element one at a time, starting with the elements that appear in the fewest compounds.
a) Balance Iron (Fe) by placing a coefficient of 3 in front of Fe(s) on the product side.
Element | Fe2O3 | CO | 3Fe | CO2
---------------------------------------
Iron (Fe) | 2 | 0 | 3 | 0
Carbon (C) | 0 | 1 | 0 | 1
Oxygen (O) | 3 | 0 | 0 | 2
b) Balance Oxygen (O) by placing a coefficient of 3/2 in front of CO(g) on the reactant side.
Element | 3/2Fe2O3 | CO | 3Fe | CO2
------------------------------------------
Iron (Fe) | 2 | 0 | 3 | 0
Carbon (C) | 0 | 1 | 0 | 1
Oxygen (O) | 9/2 | 0 | 0 | 2
c) Balance Carbon (C) by placing a coefficient of 3 in front of CO(g) on the reactant side.
Element | 3/2Fe2O3 | 3CO | 3Fe | CO2
---------------------------------------------
Iron (Fe) | 2 | 0 | 3 | 0
Carbon (C) | 0 | 3 | 0 | 3
Oxygen (O) | 9/2 | 0 | 0 | 2
Step 3: Multiply all coefficients by 2 to get rid of any fractions.
2(3/2Fe2O3) + 2(3CO) -> 2(3Fe) + 2(CO2)
3Fe2O3 + 6 CO -> 6Fe + 2CO2
Now the equation is balanced.
To find the number of moles of CO required, use the balanced coefficients as the stoichiometric ratios:
For every 6 moles of CO, 3 moles of Fe2O3 react.
So, to react 4.00 kg (4000 g) of Fe2O3, we use the molar mass of Fe2O3 to convert grams to moles:
Molar mass of Fe2O3 = 2(55.85 g/mol) + 3(16.00 g/mol) = 159.7 g/mol
Moles of Fe2O3 = (4000 g) / (159.7 g/mol) = 25.06 mol
From the balanced equation, for every 3 moles of Fe2O3, we need 6 moles of CO.
Moles of CO needed = (25.06 mol Fe2O3) * (6 mol CO / 3 mol Fe2O3) = 50.12 mol CO
Therefore, 50.12 moles of CO are needed for the reaction.
To find the moles of each product formed, use the stoichiometric ratios from the balanced equation:
From the balanced equation, for every 3 moles of Fe2O3, we produce 6 moles of Fe.
Moles of Fe formed = (25.06 mol Fe2O3) * (6 mol Fe / 3 mol Fe2O3) = 50.12 mol Fe
From the balanced equation, for every 3 moles of Fe2O3, we produce 2 moles of CO2.
Moles of CO2 formed = (25.06 mol Fe2O3) * (2 mol CO2 / 3 mol Fe2O3) = 16.71 mol CO2
Hence, 50.12 moles of Fe and 16.71 moles of CO2 are formed.
Fe2O3(s) + 2CO(g)-->2Fe(s)+ 2CO2(g)
Convert 4.00 kg Fe2O3 to moles. moles = grams/molar mass.
Now look at the balanced equation. 1 mole Fe2O3 requires 2 moles CO and produces 2 moles Fe and 2 moles CO2.