Given the balanced equation:
a. Fe2O3+3C=2Fe+3CO:
b. How many moles of Fe are produced when 1.36 moles of carbon monoxide are produced?
c. How many grams of Fe is part b equal to?
d. how many molecules of Fe are in part B
To answer these questions, we need to use the balanced equation provided. Let's walk through each step:
a. The balanced equation:
Fe2O3 + 3C = 2Fe + 3CO
b. Finding moles of Fe produced:
From the balanced equation, we can see that 1 mole of Fe is produced for every 3 moles of carbon monoxide (CO) produced. Therefore, we can set up a proportion based on the stoichiometry of the reaction:
(1 mole Fe) / (3 moles CO) = (x moles Fe) / (1.36 moles CO)
Cross-multiplying, we get:
x = (1 mole Fe) * (1.36 moles CO) / (3 moles CO)
x ≈ 0.45 moles Fe
Therefore, when 1.36 moles of carbon monoxide are produced, approximately 0.45 moles of iron (Fe) are produced.
c. Converting moles of Fe to grams:
To convert moles of Fe to grams, we need to use the molar mass of iron (Fe). The molar mass of Fe is approximately 55.845 g/mol.
Using the formula:
Grams = Moles * Molar Mass
Grams of Fe produced = 0.45 moles Fe * 55.845 g/mol ≈ 25.13 grams Fe
Therefore, 1.36 moles of carbon monoxide are equal to approximately 25.13 grams of iron (Fe).
d. Finding the number of molecules of Fe:
To find the number of molecules of Fe, we need to use Avogadro's number, which states that 1 mole of any substance contains 6.022 x 10^23 molecules.
Number of Molecules = Moles of Fe * Avogadro's Number
Number of Molecules of Fe = 0.45 moles Fe * 6.022 x 10^23 molecules/mol
Number of Molecules of Fe ≈ 2.71 x 10^23 molecules
Therefore, when 1.36 moles of carbon monoxide are produced, there are approximately 2.71 x 10^23 molecules of iron (Fe).
a. is balanced. good work.
b. 1.36 mols C x (2 mols Fe/3 mol C) = 1.36 x 2/3 = ? Note that it is all in the coefficients.
c. g = mols x atomic mass
d. 1 mol Fe contains 6.02E23 molecules so .....