The number of mole of nitrogen gas, N₂, needed to produce 150 g of ammonia, NH₃ is 4.41 moles
<h3>How to determine the mole of NH₃ produced </h3>
- Mass of NH₃ = 150 g
- Molar mass of NH₃ = 14 + (3×1) = 17 g/mol
Mole = mass /molar mass
Mole of NH₃ = 150 / 17
Mole of NH₃ = 8.82 moles
<h3>How to determine the mole of N₂ needed </h3>
Balanced equation
N₂ + 3H₂ —> 2NH₃
From the balanced equation above,
2 moles of NH₃ were produced by 1 mole of N₂.
Therefore,
8.82 moles of NH₃ will be produced by = 8.82 / 2 = 4.41 moles of N₂.
Thus, 4.41 moles of N₂ is needed for the reaction.
Learn more about stoichiometry:
brainly.com/question/14735801
The reaction 4al (s) 3o2 (
g. → 2al2o3 (s) δh° = -3351 kj is exothermic________, and therefore heat is _____release ___ by the reaction.
2) Increasing the rate of the reverse reaction will cause a shift to the left.
Hopefully, If it is wrong my full apologies.
OR IF THATS WRONG, TRY THIS
a - Increasing the rate of the forward reaction will cause equilibrium to be more product-favored (i.e. shift to the right, not the left)
Answer:
During the process of glycolysis in cellular respiration, glucose is oxidized to carbon dioxide and water. Energy released during the reaction is captured by the energy-carrying molecule ATP (adenosine triphosphate).
