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?
Duplicate post.
To determine the number of moles of reactants and products in the given reaction, we need to first calculate the molar masses of CaO and NH4Cl.
The molar mass of CaO (calcium oxide) can be calculated as follows:
CaO = 40.08 g/mol (molar mass of Ca) + 16.00 g/mol (molar mass of O)
CaO = 56.08 g/mol
The molar mass of NH4Cl (ammonium chloride) can be calculated as follows:
NH4Cl = 14.01 g/mol (molar mass of N) + 4 * 1.01 g/mol (molar mass of H) + 35.45 g/mol (molar mass of Cl)
NH4Cl = 53.49 g/mol
Next, we can calculate the number of moles for each substance using the given masses and molar masses.
Number of moles of CaO = mass of CaO / molar mass of CaO
Number of moles of CaO = 112 g / 56.08 g/mol
Number of moles of CaO = 2 moles
Number of moles of NH4Cl = mass of NH4Cl / molar mass of NH4Cl
Number of moles of NH4Cl = 224 g / 53.49 g/mol
Number of moles of NH4Cl = 4 moles
According to the balanced equation, the molar ratio of CaO to NH4Cl is 1:2. Therefore, the number of moles of CaO is twice the number of moles of NH4Cl.
Now, let's calculate the number of moles of products based on the stoichiometry of the balanced equation.
Using the balanced equation CaO(s) + 2NH4Cl(s) -> 2NH3(g) + H2O(g) + CaCl2(s), we can see that the molar ratio of CaO to NH3 is 1:2.
Number of moles of NH3 = 2 moles of NH4Cl (since NH4Cl reacts in 1:2 ratio with NH3)
Number of moles of NH3 = 2 moles
Therefore, the number of moles of reactants and products when the reaction is complete are as follows:
Reactants:
- CaO: 2 moles
- NH4Cl: 4 moles
Products:
- NH3: 2 moles
- H2O: 2 moles
- CaCl2: 2 moles
To determine the number of moles of reactants and products, we need to follow the steps below:
Step 1: Convert the given masses of substances to moles.
First, we calculate the number of moles of CaO:
1. Calculate the molar mass of CaO:
- Molar mass of Ca = 40.08 g/mol
- Molar mass of O = 16.00 g/mol
- Molar mass of CaO = 40.08 g/mol + 16.00 g/mol = 56.08 g/mol
2. Convert the mass of CaO to moles:
- Moles of CaO = Mass of CaO / Molar mass of CaO
- Moles of CaO = 112 g / 56.08 g/mol = 2 moles
Next, we calculate the number of moles of NH4Cl:
1. Calculate the molar mass of NH4Cl:
- Molar mass of N = 14.01 g/mol
- Molar mass of H = 1.01 g/mol
- Molar mass of Cl = 35.45 g/mol
- Molar mass of NH4Cl = 14.01 g/mol + (1.01 g/mol × 4) + 35.45 g/mol = 53.49 g/mol
2. Convert the mass of NH4Cl to moles:
- Moles of NH4Cl = Mass of NH4Cl / Molar mass of NH4Cl
- Moles of NH4Cl = 224 g / 53.49 g/mol = 4.18 moles
Step 2: Determine the mole ratio between the reactants and products.
From the balanced chemical equation, we can see that the mole ratio between CaO and NH4Cl is 1:2. This means that for every 1 mole of CaO, we need 2 moles of NH4Cl to react completely.
Step 3: Calculate the number of moles of products using the mole ratio.
Using the mole ratio, we can calculate the number of moles of products formed when the reaction is complete:
1. Moles of NH3 = Moles of NH4Cl × (2 moles NH3 / 1 mole NH4Cl) = 4.18 moles × 2 = 8.36 moles
2. Moles of H2O = Moles of NH4Cl × (1 mole H2O / 1 mole NH4Cl) = 4.18 moles × 1 = 4.18 moles
3. Moles of CaCl2 = Moles of CaO × (1 mole CaCl2 / 1 mole CaO) = 2 moles × 1 = 2 moles
Therefore, when the reaction is complete, there are:
- 2 moles of CaO
- 4.18 moles of NH4Cl
- 8.36 moles of NH3
- 4.18 moles of H2O
- 2 moles of CaCl2