Question

NCl3 + 3H20 - NH3 + 3HCIO

How many grams of ammonia can be produced from 1.33 grams of nitrogen trichloride?

Answer 1

To find out how many grams of ammonia can be produced from 1.33 grams of nitrogen trichloride, we can use stoichiometry.

Step-by-step explanation:

To find out how many grams of ammonia can be produced from 1.33 grams of nitrogen trichloride, we need to use stoichiometry. The balanced equation is NCl3 + 3H2O → NH3 + 3HCl.

We can use the molar mass of NCl3 to convert grams to moles, then use the stoichiometric ratio between NCl3 and NH3 to find the number of moles of NH3 produced. Finally, we can convert moles of NH3 to grams using the molar mass of NH3.

Given that the molar mass of NCl3 is 51.49 g/mol and the molar mass of NH3 is 17.03 g/mol, we can calculate:

1.33 g NCl3 * (1 mol NCl3 / 51.49 g NCl3) * (1 mol NH3 / 1 mol NCl3) * (17.03 g NH3 / 1 mol NH3) = X g NH3

The answer will be the value of X.

Answer 2

0.189 g

Step-by-step explanation:

Step 1: Write the balanced equation

NCl₃ + 3 H₂O ⇒ NH₃ + 3 HCIO

Step 2: Calculate the moles corresponding to 1.33 g of NCl₃

The molar mass of NCl₃ is 120.36 g/mol.

1.33 g × 1 mol/120.36 g = 0.0111 mol

Step 3: Calculate the moles of NH₃ produced from 0.0111 moles of NCl₃

The molar ratio of NCl₃ to NH₃ is 1:1. The moles of NH₃ produced are 1/1 × 0.0111 mol = 0.0111 mol.

Step 4: Calculate the mass corresponding to 0.0111 moles of NH₃

The molar mass of NH₃ is 17.03 g/mol.

0.0111 mol × 17.03 g/mol = 0.189 g