What is the volume of 0.5 moles of a gas at 2 atmospheres of pressure and 15°c
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Answer:
The value of the partial pressure of the oxygen = 690 torr
Explanation:
Total pressure of the mixture of gases = 736 torr
The partial pressure of water vapor = 46 torr
From the law of pressure we know that
Total pressure = The partial pressure of water vapor + The partial pressure of oxygen
Put the values of pressures in above equation we get,
⇒ 736 = 46 +
⇒ = 736 - 46
⇒ = 690 torr
This is the value of the partial pressure of the oxygen.
The volume of 0. 250 m sulfuric acid solution would be needed to react completely with 18. 00 ml of 0. 350 m ammonia solution is 0.0504 L.
The balance reaction is 2KOH+=
This shows us that we need 2 moles of KOH for each mole of sulfuric acid.
So, we write mathematically 2*(0.018*0.350)=(V*0.250)
V=(2*0.018*0.350)/0.250=0.0504 L
<h3>Sulfuric acid</h3>With the chemical formula H2SO4, sulfuric acid, also known as sulphuric acid or oil of vitriol, is a mineral acid made up of the elements hydrogen, oxygen, and sulfur. It is a viscous liquid that is miscible with water and is colorless, odorless, and viscous.
Since pure sulfuric acid has a significant affinity for water vapor, it does not naturally occur on Earth; as a result, it is hygroscopic and rapidly collects water vapor from the atmosphere. Due to its potent dehydrating and oxidizing qualities, concentrated sulfuric acid is extremely corrosive to various materials, including rocks and metals. One significant exception is phosphorus pentoxide, which dehydrates sulfuric acid to sulfur trioxide instead of being dehydrated by sulfuric acid.
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