Answer:
Propane
Explanation:
From the question given, we were told that 0.1240 kg of propane reacted with excess oxygen to produce 0.3110kg of carbon dioxide.
Since the reaction took place in the presence of excess oxygen, therefore, propane is the limiting reactant as all of it is used up in the presence of excess oxygen.
I think you're talking about Ribosomes?
This is the organelle responsible for protein synthesis.
The pressure of the oxygen gas collected : 718 mmHg
<h3>Further explanation</h3>
Given
P tot = 748 mmHg
P water vapour = 30 mmHg
Required
P Oxygen
Solution
Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Can be formulated:
P tot = P1 + P2 + P3 ....
The partial pressure is the pressure of each gas in a mixture
P tot = P H₂O + P Oxygen
P Oxygen = 748 mmHg - 30 mmHg
P Oxygen = 718 mmHg
Explanation:
carbon dioxide has a percent composition of 72.7% oxygen, i.e. for every 100 g of carbon dioxide you get 72.7 g of oxygen.
Answer:
The balanced equation for the complete oxidation reaction uses 2 moles of butane and 13 moles of Oxygen.
Explanation:
The oxidation of butane is shown in the following picture. As it is a complete combustion, the products of this reaction are carbon dioxide and water.
