Question

using the same amount of ammonium nitrate 20 g how much water is formed

Answer 1

To calculate the amount of water formed when 20 g of ammonium nitrate decomposes, we need to consider the balanced chemical equation for the reaction:

NH4NO3(s) ⟶ 2H2O(g) + N2O(g)

According to the equation, the molar ratio between ammonium nitrate and water is 1:2.

The molar mass of ammonium nitrate (NH4NO3) is:
(1 × 14.01 g/mol) + (4 × 1.01 g/mol) + 14.01 g/mol + (3 × 16.00 g/mol) = 80.05 g/mol

Therefore, 20 g of ammonium nitrate is equal to:
20 g / 80.05 g/mol = 0.2499 mol

Since the ratio between ammonium nitrate and water is 1:2, we can multiply the number of moles of ammonium nitrate by 2 to find the moles of water formed:

0.2499 mol × 2 = 0.4998 mol

Finally, to convert the moles of water into grams, we need to multiply by the molar mass of water:

0.4998 mol × 18.02 g/mol = 8.993 g

Therefore, when 20 g of ammonium nitrate decomposes, approximately 8.993 g of water is formed.