4 mol / 205g H2O = 4/.205 = 19.5 mol/kg boiling point = 100 + 19.5 • 0.51 = 109 ºC
Answer:
True
Explanation:
This is because, The hydroboration oxidation of an alkene which is isobutene in the presence of a catalyst will result to alcohol as the product . Therefore, the OH group will attach or link itself to the carbon which is less obstructed. Thus this reaction is in accordance to Anti-Markownikoff's rule.
So isobutene on hydroboration oxidation will produce ter isobutyl alcohol.
I think the molecular formula would be CHO.
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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
Answer:
<u>~</u><u>Law of Conservation of </u><u>energy~</u>
The law of conservation of energy states that energy can neither be created nor destroyed, only energy can be converted from one form to another.
