<h3>Answer:</h3>
<u>∅</u><u>C</u>. The amount of energy required to turn a mole of a liquid into a gas
<h3>Explaination:</h3>
The amount of energy required to convert a liquid to a gas is called the enthalpy of vaporization
┌─────── ∘°❁°∘ ───────┐
︎ CarryOnLearning ૮₍˶ᵔ ᵕ ᵔ˶₎ა
︎︎└─────── °∘❁∘° ───────┘
To calculate the <span>δ h, we must balance first the reaction:
NO + 0.5O2 -----> NO2
Then we write all the reactions,
2O3 -----> 3O2 </span><span>δ h = -426 kj eq. (1)
O2 -----> 2O </span><span>δ h = 490 kj eq. (2)
NO + O3 -----> NO2 + O2 </span><span>δ h = -200 kj eq. (3)
We divide eq. (1) by 2, we get
</span>O3 -----> 1.5O2 δ h = -213 kj eq. (4)
Then, we subtract eq. (3) by eq. (4)
NO + O3 -----> NO2 + O2 δ h = -200 kj
- (O3 -----> 1.5 O2 δ h = -213 kj)
NO -----> NO2 - 0.5O2 δ h = 13 kj eq. (5)
eq. (2) divided by -2. (Note: Dividing or multiplying by negative number reverses the reaction)
O -----> 0.5O2 <span>δ h = -245 kj eq. (6)
</span>
Add eq. (6) to eq. (5), we get
NO -----> NO2 - 0.5O2 δ h = 13 kj
+ O -----> 0.5O2 δ h = -245 kj
NO + O ----> NO2 δ h = -232 kj
<em>ANSWER:</em> <em>NO + O ----> NO2 δ h = -232 kj</em>
This
can be solved using Dalton's Law of Partial pressures. This law states that the
total pressure exerted by a gas mixture is equal to the sum of the partial
pressure of each gas in the mixture as if it exist alone in a container. In
order to solve, we need the partial pressures of the gases given. Calculations
are as follows:<span>
<span>P = 3.00 atm + 1.80 atm + 0.29 atm + 0.18 atm + 0.10 atm</span></span>
<span><span>P = 5.37 atm</span></span>
A2+. Group 2 elements form cations with 2+ charge.
Answer:
reproduction
Explanation:
reproduction, process by which organisms replicate themselves
