1.00 g zinc and 0.80 g sulfur are allowed to react all the zinc is used up 1.50 g of zinc sulfide is formed and some unreacted sulfur remains what is the mass of unreacted sulfur
Zn + S ==> ZnS
mols Zn = 1.00/65.39 = 0.016 but you need to do it more accurately.
Convert mols Zn to mols S. That's 0.016 mols Zn x (1 mol S/1 mol Zn) = 0.016 mols Zn x 1/1 = 0.016 mols S.
grams S used = mols x atomic mass S; then
g S initially - g S used = g S remaining after the reaction.
.30 g
To find the mass of unreacted sulfur, we need to determine the amount of sulfur that reacted with zinc to form zinc sulfide. Then, we can subtract this amount from the initial mass of sulfur to find the mass of unreacted sulfur.
First, let's calculate the molar mass of zinc (Zn) and sulfur (S):
- Molar mass of Zn = 65.38 g/mol
- Molar mass of S = 32.06 g/mol
Next, we'll use stoichiometry to find the amount of sulfur that reacted with zinc in the balanced chemical equation:
Zn + S → ZnS
According to the equation, 1 mole of zinc reacts with 1 mole of sulfur to form 1 mole of zinc sulfide.
The amount of zinc used can be calculated using its molar mass:
Mass of Zn = 1.00 g
Moles of Zn = Mass of Zn / Molar mass of Zn
Moles of Zn = 1.00 g / 65.38 g/mol = 0.0153 mol
Since the reaction is 1:1 between zinc and sulfur, the moles of sulfur used will also be 0.0153 mol.
To find the mass of sulfur used, we multiply the moles of sulfur by its molar mass:
Mass of S used = Moles of S × Molar mass of S
Mass of S used = 0.0153 mol × 32.06 g/mol = 0.491 g
Finally, to calculate the mass of unreacted sulfur, we subtract the mass of sulfur used from the initial mass of sulfur:
Mass of unreacted S = Initial mass of S - Mass of S used
Mass of unreacted S = 0.80 g - 0.491 g = 0.309 g
Therefore, the mass of unreacted sulfur is 0.309 grams.
To find the mass of unreacted sulfur, we need to determine the amount of sulfur that reacted with the zinc and subtract it from the total initial mass of sulfur.
First, we need to calculate the number of moles of zinc and sulfur using their respective molar masses:
1. Find the molar mass of zinc (Zn):
- The atomic mass of zinc (Zn) is 65.38 g/mol.
2. Calculate the number of moles of zinc (nZn):
- nZn = mass of zinc / molar mass of zinc
- nZn = 1.00 g / 65.38 g/mol
3. Find the molar mass of sulfur (S):
- The atomic mass of sulfur (S) is 32.06 g/mol.
4. Calculate the number of moles of sulfur (nS):
- nS = mass of sulfur / molar mass of sulfur
- nS = 0.80 g / 32.06 g/mol
Next, we need to determine the balanced chemical equation for the reaction between zinc and sulfur:
Zn + S -> ZnS
1 mole of zinc reacts with 1 mole of sulfur to form 1 mole of zinc sulfide.
Since the ratio between zinc and sulfur is 1:1, the moles of zinc reacted will be the same as the moles of sulfur reacted.
Now, we can find the moles of sulfur that reacted using the moles of zinc calculated earlier:
5. Moles of sulfur reacted (nS_reacted) = Moles of zinc reacted (nZn)
Finally, we can calculate the mass of unreacted sulfur using the moles of sulfur reacted:
6. Mass of unreacted sulfur = Total mass of sulfur - Mass of sulfur reacted
- Mass of sulfur reacted = nS_reacted * molar mass of sulfur
Plug in the values calculated earlier to get the final answer.