4NH3+5O2=4NO+6H20 if 32.5 grams of NH3 react with enough oxygen, how many grams of water should form?
1 answer:
51.3 gram of water should form if 32.5 g of NH₃ react with enough oxygen.
<h3>How to find the Number of moles ?</h3>To calculate the number of moles use the formula
Number of moles =
=
= 1.9 mol
4NH₃ + 5O₂ → 4NO + 6H₂O
4 mol of NH₃ react with oxygen to given 6 mole of water.
So 1.9 mol of NH₃ produces =
= 2.85 mol of water
Mass of water = Molar Mass of water × Number of moles of water
= 18 × 2.85
= 51.3 gram
Thus from the above conclusion we can say that 51.3 gram of water should form if 32.5 g of NH₃ react with enough oxygen.
Learn more about the Moles here: brainly.com/question/15356425
#SPJ1
You might be interested in
Answer: The correct option is (c). The total pressure doubles.
Solution:
Initially, only 4 moles of oxygen gas were present in the flask.
(
) ( according to Dalton's law of partial pressure)
....(1)
= Total pressure when only oxygen gas was present.
Final total pressure when 4 moles of helium gas were added:
partial pressure of oxygen in the mixture :
Since, the number of moles of oxygen remains the same, the partial pressure of oxygen will also remain the same in the mixture.
= Total pressure of the mixture.
from (1)
On rearranging, we get:
The new total pressure will be twice of initial total pressure.