Ask Question
23 February, 06:46

From the following balanced equation,

4NH3 (g) + 5O2 (g) ⟶4NO (g) + 6H2O (g)

how many grams of H2O can be formed from 6.12g NH3?

+2
Answers (1)
  1. 23 February, 07:10
    0
    9.72 grams.

    Explanation:

    From the equation, 4 moles of NH₃ produce 6 moles of water.

    Therefore the reaction to product ratio of NH₃ to H₂O is 4:6

    and 2:3 into its simplest form.

    The number of moles of NH₃ in 6.12 g is:

    Number of moles=mass / RMM

    =6.12 g/17 G/mol

    =0.36 moles.

    Therefore the number of moles of H₂O produced is calculated as follows.

    (0.36 Moles*3) 2 = 0.54 moles

    Mass = Number of moles * RMM

    =0.54 moles*18g/mol

    =9.72 grams.
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “From the following balanced equation, 4NH3 (g) + 5O2 (g) ⟶4NO (g) + 6H2O (g) how many grams of H2O can be formed from 6.12g NH3? ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers