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)
mols Sb2S3 = 3.87E23/6.02E23 = ?
Then mols Sb2S3 x (3 mols FeS/1 mol Sb2S3) = ?
Finally, grams = mols x molar mass
Well, let's start by calculating the molar mass of FeS. Fe has a molar mass of 55.845 g/mol, and S has a molar mass of 32.06 g/mol. So the molar mass of FeS would be 55.845 + (32.06*1) = 87.905 g/mol.
Now, using the stoichiometry of the balanced equation, we can determine the number of moles of FeS produced. For every 3 moles of Fe, we get 3 moles of FeS. Therefore, the number of moles of FeS would be equal to the moles of Sb2S3 divided by 3.
To find the number of moles of Sb2S3, we can use Avogadro's number (6.022 × 10^23) and the given amount of particles (3.87 × 10^23). So, the number of moles of Sb2S3 would be 3.87 × 10^23 particles / 6.022 × 10^23 particles/mol.
Calculating this, we get:
Moles of Sb2S3 = 3.87 × 10^23 / 6.022 × 10^23 = 0.643 mol
Since the molar ratio between FeS and Sb2S3 is 3:1, we can multiply the number of moles of FeS by the molar mass of FeS to find the mass of FeS produced.
Mass of FeS = 0.643 mol * 87.905 g/mol = 56.58 g
Therefore, approximately 56.58 grams of FeS would be produced. But hey, don't be too scared! It's just some iron and sulfur having a little party!
To determine the mass of FeS(s) produced, we need to use the balanced equation to calculate the molar ratio between Sb2S3(s) and FeS(s), and then use the molar mass of FeS(s) to convert the number of moles of FeS(s) to grams.
Let's start with the balanced equation:
Sb2S3(s) + 3Fe(s) → 2Sb(s) + 3FeS(s)
The balanced equation tells us that the ratio between Sb2S3(s) and FeS(s) is 1:3. This means that for every 1 mole of Sb2S3(s) reacted, 3 moles of FeS(s) are produced.
Step 1: Calculate the number of moles of Sb2S3(s) reacted.
Given: 3.87×10^23 particles of Sb2S3(s)
To convert particles to moles, we need to divide the number of particles by Avogadro's number (6.022 × 10^23).
3.87×10^23 particles / 6.022 × 10^23 particles/mole = 0.642 moles of Sb2S3(s) reacted
Step 2: Use the molar ratio to calculate the number of moles of FeS(s) produced.
According to the balanced equation, the ratio between Sb2S3(s) and FeS(s) is 1:3.
Therefore, the number of moles of FeS(s) produced is:
0.642 moles of Sb2S3(s) x (3 moles of FeS(s)/1 mole of Sb2S3(s)) = 1.927 moles of FeS(s) produced
Step 3: Calculate the mass of FeS(s) produced.
The molar mass of FeS(s) is the sum of the atomic masses of Fe and S.
Fe: 55.845 g/mol
S: 32.06 g/mol
FeS: 55.845 g/mol + 32.06 g/mol = 87.905 g/mol
To convert the number of moles of FeS(s) to grams, multiply by the molar mass:
1.927 moles of FeS(s) x 87.905 g/mol = 169.44 grams of FeS(s) produced
Therefore, the mass of FeS(s) produced is 169.44 grams.
To find the mass of FeS(s) produced, we need to use stoichiometry and the given number of particles.
Step 1: Find the molar ratio between Sb2S3 and FeS
From the balanced chemical equation, we can see that the ratio of Sb2S3 to FeS is 1:3. This means that for every 1 mole of Sb2S3 reacted, 3 moles of FeS are produced.
Step 2: Convert the given number of particles of Sb2S3 to moles
The given number of particles of Sb2S3 is 3.87×10^23. To convert this to moles, we need to divide by Avogadro's number (6.022×10^23 particles/mol).
Number of moles of Sb2S3 = (3.87×10^23 particles) / (6.022×10^23 particles/mol)
Step 3: Calculate the number of moles of FeS produced
Since the ratio between Sb2S3 and FeS is 1:3, the number of moles of FeS produced is 3 times the number of moles of Sb2S3.
Number of moles of FeS = (Number of moles of Sb2S3) * 3
Step 4: Convert moles of FeS to mass
To convert the moles of FeS to mass, we need to multiply by the molar mass of FeS. The molar mass of FeS is calculated by adding the atomic masses of iron (Fe) and sulfur (S).
Molar mass of FeS = (molar mass of Fe) + (molar mass of S)
Step 5: Calculate the mass of FeS
Mass of FeS = (Number of moles of FeS) * (Molar mass of FeS)
Following these steps, you can calculate the mass of FeS produced.