The combustion of ammonia in presence of excess oxygen yields NO2 and H2O.
The molar mass of ammonia is 17.02 g/mol
Therefore, moles of ammonia in 43.9 g
= 43.9 /17.02
= 2.579 moles
From the equation the mole ratio of ammonia to nitrogen iv oxide is 4:4
The molar mass of NO2 is 46 g/mol
The number of moles of NO2 is the same as that of ammonia since they have equal ratio,
= 2.579 moles
Therefore, mass of NO2
= 2.579 moles ×46
= 118.634 g
≈ 119 g
Answer:
hydration reaction
Explanation:
The type of reaction would be hydration reaction.
<u>Hydration reaction generally involves a chemical reaction of water with another reactant and in which the water ends up being converted to another product entirely. </u>
A good example of hydration reaction is the reaction between alkene and water leading to the production of alcohol.
⇄ 
Multiply avagadro’s number to the mole
(6.022x10^22) x (0.026)=1.565 x 10^22
Answer:
weak bonds require less energy to form bonds than strong bonds
