What amount (in moles) of FeS2(s) are required to produced 64g of SO2(g) according to the following equation?
4FeS2(s) + 110(g)_________2FeO3(s)__8SO2(g)...remember the first long bar is an arrow.
To determine the amount of FeS2(s) required, we need to use the stoichiometry of the given balanced equation.
The balanced equation is:
4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g)
From the equation, we can see that:
4 moles of FeS2 produce 8 moles of SO2
Now, let's calculate the moles of SO2 produced from the given mass of 64g:
1 mole of SO2 has a molar mass of 64g/mol. Therefore, 64g of SO2 is equal to:
64g SO2 × (1 mol SO2 / 64g SO2) = 1 mol SO2
Since 4 moles of FeS2 produce 8 moles of SO2, we can set up a ratio using the stoichiometric coefficients from the equation:
4 mol FeS2 / 8 mol SO2
Now, we can calculate the moles of FeS2 required:
1 mol SO2 × (4 mol FeS2 / 8 mol SO2) = 0.5 mol FeS2
Therefore, 0.5 moles of FeS2(s) are required to produce 64g of SO2(g) according to the given equation.
To find the amount of FeS2 (in moles) required to produce 64g of SO2 according to the given equation, we need to follow these steps:
Step 1: Balance the equation
The balanced equation is:
4FeS2(s) + 11O2(g) -> 2Fe2O3(s) + 8SO2(g)
Step 2: Calculate the molar mass
The molar mass of FeS2 is calculated as follows:
Molar mass(FeS2) = (1 mol Fe × atomic mass of Fe) + (2 mol S × atomic mass of S)
Molar mass(FeS2) = (1 × 55.85 g/mol) + (2 × 32.07 g/mol)
Molar mass(FeS2) = 119.99 g/mol
Step 3: Convert grams of SO2 to moles
We are given that the mass of SO2 is 64g. To convert this to moles, we use the molar mass of SO2, which is 32.07 g/mol.
Moles of SO2 = mass of SO2 / molar mass of SO2
Moles of SO2 = 64g / 32.07 g/mol
Moles of SO2 = 1.995 mol
Step 4: Use the stoichiometry of the balanced equation to find moles of FeS2
By comparing the coefficients in the balanced equation, we can see that the stoichiometric ratio between FeS2 and SO2 is 4:8 (or 1:2).
Thus, the moles of FeS2 = (moles of SO2) × (4 moles of FeS2 / 8 moles of SO2)
Moles of FeS2 = 1.995 mol × 4/8
Moles of FeS2 = 0.9975 mol
Therefore, approximately 0.9975 moles of FeS2 are required to produce 64g of SO2 according to the given equation.
7.81 mol/ FeS2
Your equation doesn't make sense to me. I assume you mean something like this.
4FeS2 + 11 O2 ==> 2Fe2O3 + 8SO2
Convert 64 g SO2 to moles. moles = grams/molar mass.
Using the coefficients in the balanced equation, convert moles SO2 to moles FeS2.
Convert moles FeS2 to grams. grams = moles x molar mass.
Post your work if you get stuck.