Answer:
There are two phase changes where the heat energy is released: Condensation: When gas condenses to liquid the quantity of energy converted from chemical to heat is called the Heat of Vaporization or Δ Hvap .
At constant temperature, if the volume of the gas decreased to the given value, the pressure increases to 2.16atm.
<h3>What is Boyle's law?</h3>
Boyle's law simply states that "the volume of any given quantity of gas is inversely proportional to its pressure as long as temperature remains constant.
Boyle's law is expressed as;
P₁V₁ = P₂V₂
Where P₁ is Initial Pressure, V₁ is Initial volume, P₂ is Final Pressure and V₂ is Final volume.
Given the data in the question question;
- Initial volume of the gas V₁ = 682mL = 0.682L
- Initial pressure of the gas P₁ = 1.33atm
- Final volume of the gas V₂ = 0.419L
- Final pressure of the gas P₂ = ?
P₁V₁ = P₂V₂
P₂ = P₁V₁ / V₂
P₂ = ( 1.33atm × 0.682L) / 0.419L
P₂ = 0.90706Latm / 0.419L
P₂ = 2.16atm
Therefore, at constant temperature, if the volume of the gas decreased to the given value, the pressure increases to 2.16atm.
Learn more about Boyle's law here: brainly.com/question/1437490
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It increases because the electrons are held tighter together by the higher effective nuclear charge. The electrons are held in lower energy orbitals and closer to the nucleus and more tightly bound and harder to remove from the atom.
Answer 1) Option A) 58.05
In the given reaction of iron forming rust when reacts with the oxygen.
We can clearly see that, 4 moles of iron reacts with 3 moles of oxygen to give 2 moles of iron oxide.
So 4 Fe : 3 O and 77.4 moles of Fe : x moles of O
(3 X 77.4) / 4 = 58.05
So when we solve we get x as 58.05.
Hence the no. of moles of oxygen will be 58.
Answer 2) Option A) 10.03
The number of moles of carbon dioxide produced when 161.0 g of methane undergoes combustion will be 10.03
as we know the molar mass of methane is 16.043
g
As we can see in the reaction the mole ratio is 1:1;
1 mole of methane produces 1 mole of carbondioxide.
So, 161 g / 16.043 g = 10.03 moles of Carbon dioxide.
