Given the equation below, if 3.87×1023 particles of Sb2S3(s) are reacted with excess Fe(s), what mass of FeS(s) is produced?
Sb2S3(s) + 3Fe(s)→2Sb(s) +3FeS(s)
168g
To find the mass of FeS(s) produced, we need to use stoichiometry. Stoichiometry is the calculation of quantitative relationships between reactants and products in a chemical reaction.
Step 1: Identify the balanced equation
The balanced equation states that 1 mole of Sb2S3 reacts with 3 moles of Fe to produce 3 moles of FeS.
Step 2: Calculate the moles of Sb2S3
Given that the number of particles of Sb2S3 is 3.87 × 10^23, we can find the moles of Sb2S3 by dividing the number of particles by Avogadro's number (6.022 × 10^23 particles/mol).
Moles of Sb2S3 = 3.87 × 10^23 particles / 6.022 × 10^23 particles/mol
Step 3: Use stoichiometry to find moles of FeS
From the balanced equation, we know that 1 mole of Sb2S3 results in 3 moles of FeS. Therefore, the moles of FeS produced will be equal to the moles of Sb2S3.
Moles of FeS = Moles of Sb2S3
Step 4: Calculate the mass of FeS
To find the mass of FeS, we need to know the molar mass of FeS. The molar mass of FeS can be found by adding the atomic masses of iron (Fe) and sulfur (S) together from the periodic table.
Molar mass of FeS = Atomic mass of Fe + Atomic mass of S
Finally, to find the mass of FeS:
Mass of FeS = Moles of FeS × Molar mass of FeS
By following these steps, you can solve the problem. Remember to use the appropriate units and round your answer to the correct number of significant figures.