Ion arrangements of three general salts are represented below. h5sil917 h5sil917021 h5sil91703 which ion arrangement has the hig
hest lattice energy
1 answer:
This question is incomplete. Luckily, I found the same problem which is shown in the attached picture. To answer the question, we must know how the size and charge affect the lattice energy. The answer is: lattice energy increases with the increasing charge of the ions, and decreasing radius of the atoms. <em>Therefore, the ranking would be: A < B < C</em>.
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Answer:
<h2>The equilibrium constant Kc for this reaction is 19.4760</h2>Explanation:
The volume of vessel used= ml
Initial moles of NO= moles
Initial moles of H2= moles
Concentration of NO at equilibrium= M
Moles of NO at equilibrium=
= moles
2H2 (g) + 2NO(g) <—> 2H2O (g) + N2 (g)
<u>Initial</u> :1.3*10^-2 2.6*10^-2 0 0 moles
<u>Equilibrium</u>:1.3*10^-2 - x 2.6*10^-2-x x x/2 moles
∴
⇒
<u>Equilibrium</u>:0.31*10^-2 1.61*10^-2 0.99*10^-2 0.495*10^-2 moles
⇒
⇒
Answer:
The equilibrium temperature of the system is 276.494 Kelvin.
Explanation:
Let consider the system formed by the sample of aluminium and water as a control mass, in which the sample is cooled and water is heated until thermal equilibrium is reached. The energy process is represented by First Law of Thermodynamics:
Where:
- Heat received by water, measured in joules.
- Heat released by the sample of aluminium, measured in joules.
Given that no mass is evaporated, the previous expression is expanded to:
Where:
,
- Mass of water and the sample of aluminium, measured in kilograms.
,
- Specific heats of the sample of aluminium and water, measured in joules per kilogram-Kelvin.
,
- Initial temperatures of the sample of aluminium and water, measured in Kelvin.
- Temperature which system reaches thermal equilibrium, measured in Kelvin.
The final temperature is now cleared:
Given that ,
,
,
,
and
, the final temperature of the system is:
The equilibrium temperature of the system is 276.494 Kelvin.