Ammonia gas can be prepared by the reaction CaO(s) + 2NH4Cl(s) -> 2NH3(g) + H2O(g) + CaCl2(s)
If 112 g CaO reacts with 224 g NH4Cl, how many moles of reactants and products are there when the reaction is complete?
quantity (g) of pure CaCl2 in 7.5g of CaCl2 9H2O
This answer is right
To determine the number of moles, we need to convert the mass of each substance to moles using their respective molar masses.
1. CaO:
The molar mass of CaO is 40.08 g/mol.
We can calculate the number of moles using the formula:
Number of moles = mass / molar mass
Number of moles of CaO = 112 g / 40.08 g/mol
Number of moles of CaO = 2.794 mol
2. NH4Cl:
The molar mass of NH4Cl is 53.49 g/mol.
Number of moles of NH4Cl = 224 g / 53.49 g/mol
Number of moles of NH4Cl = 4.189 mol
Now let's calculate the number of moles of the products:
1. NH3:
From the balanced equation, we can see that the molar ratio between NH3 and CaO is 2:1.
Therefore, the number of moles of NH3 will be equal to half the number of moles of CaO.
Number of moles of NH3 = 2.794 mol / 2
Number of moles of NH3 = 1.397 mol
2. H2O:
From the balanced equation, the molar ratio between H2O and CaO is also 1:1.
Therefore, the number of moles of H2O will be equal to the number of moles of CaO.
Number of moles of H2O = 2.794 mol
3. CaCl2:
From the balanced equation, the molar ratio between CaCl2 and CaO is also 1:1.
Therefore, the number of moles of CaCl2 will be equal to the number of moles of CaO.
Number of moles of CaCl2 = 2.794 mol
To summarize:
Number of moles of reactants:
- CaO = 2.794 mol
- NH4Cl = 4.189 mol
Number of moles of products:
- NH3 = 1.397 mol
- H2O = 2.794 mol
- CaCl2 = 2.794 mol
To determine the number of moles of reactants and products, we need to convert the given masses of CaO and NH4Cl into moles using their respective molar masses. Then, based on the balanced chemical equation, we can determine the number of moles of each substance involved in the reaction.
First, let's calculate the number of moles of CaO:
Molar mass of CaO (Ca = 40.08 g/mol, O = 16.00 g/mol) = 40.08 + 16.00 = 56.08 g/mol
Moles of CaO = Mass of CaO / Molar mass of CaO
Moles of CaO = 112 g / 56.08 g/mol
Moles of CaO = 2 mol
Next, let's calculate the number of moles of NH4Cl:
Molar mass of NH4Cl (N = 14.01 g/mol, H = 1.01 g/mol, Cl = 35.45 g/mol) = 14.01 + (4 × 1.01) + 35.45 = 53.49 g/mol
Moles of NH4Cl = Mass of NH4Cl / Molar mass of NH4Cl
Moles of NH4Cl = 224 g / 53.49 g/mol
Moles of NH4Cl = 4.19 mol (rounded to two decimal places)
From the balanced chemical equation, we can see that 1 mol of CaO reacts with 2 mol of NH4Cl to produce 2 mol of NH3, 1 mol of H2O, and 1 mol of CaCl2.
Thus, the number of moles of each substance when the reaction is complete is:
Moles of CaO = 2 mol (given)
Moles of NH4Cl = 4.19 mol (calculated)
Moles of NH3 = 2 × Moles of NH4Cl = 2 × 4.19 mol = 8.38 mol
Moles of H2O = 2 × Moles of NH4Cl = 2 × 4.19 mol = 8.38 mol
Moles of CaCl2 = 1 × Moles of CaO = 1 × 2 mol = 2 mol
Therefore, when the reaction is complete, there are 2 mol of CaO, 4.19 mol of NH4Cl, 8.38 mol of NH3, 8.38 mol of H2O, and 2 mol of CaCl2.