Answer:
82.08 %
Explanation:
- <em>The percent yield of the reaction = [(actual yield)/(calculated yield)] x 100.
</em>
Actual yield = 26.80 kg.
- <em><u>To get the calculated yield:
</u></em>
- The balanced equation of reacting N2 with H2 to produce NH3 is:
N₂ + 3H₂ → 2NH₃
- It is clear that 1.0 mole of N₂ reacts with 3.0 moles of H₂ to produce 2.0 moles of NH₃.
- N₂ is present in excess and H₂ is the limiting reactant.
- We need to convert the mass of H₂ added (5.79 kg) to moles using the relation:
n = mass /molar mass = (5790 g) / (2.01 g/mol) = 2880.6 mol.
- We can get the no. of moles of NH₃ produced.
<u><em>Using cross multiplication:
</em></u>
3.0 mole of H₂ produce → 2.0 moles off NH₃, from the stichiometry.
2880.6 mol of H₂ produces → ??? moles of NH₃.
- The no. of moles of NH₃ produced = (2880.6 mol)(2.0 mol) / (3.0 mol) = 1920.4 mol.
- We can know get the calculated yield of NH₃ = no. of moles x molar mass = (1920.4 mol) (17.00 g/mol) = 32646.76 g ≅ 32.65 kg.
∴ <em>The percent yield of the reaction = [(actual yield)/(calculated yield)] x 100 = </em>[(26.8 kg) / (32.65 kg)] x 100 <em>= 82.08 %.</em>
Answer: The correct formula for phosphorous pentachloride is 
because a subscript 5 indicates five chlorine (Cl) atoms.
Explanation: For the given molecule, phosphorous pentachloride, there are 2 atoms present which are phosphorous and chlorine atoms.
Number of phosphorous atoms = 1
Number of chlorine atoms = 5
So, the correct formula for phosphorous pentachloride will be because the subscript 5 represents the 5 chlorine atoms.
a. 0.137
b. 0.0274
c. 1.5892 g
d. 0.1781
e. 5.6992 g
<h3>Further explanation</h3>
Given
Reaction
2 C4H10 + 13O2 -------> 8CO2 + 10H2O
2.46 g of water
Required
moles and mass
Solution
a. moles of water :
2.46 g : 18 g/mol = 0.137
b. moles of butane :
= 2/10 x mol water
= 2/10 x 0.137
= 0.0274
c. mass of butane :
= 0.0274 x 58 g/mol
= 1.5892 g
d. moles of oxygen :
= 13/2 x mol butane
= 13/2 x 0.0274
= 0.1781
e. mass of oxygen :
= 0.1781 x 32 g/mol
= 5.6992 g
