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EastWind [94]
3 years ago
9

Why do atoms become anion and cations (remember the octet rule and how 8 is a very important number)?

Chemistry
1 answer:
Kryger [21]3 years ago
8 0

Answer:

The atoms become cations because they have lost electrons and the atoms and has a positive charge then atoms become a ions because they have gained electrons from cations and has a negative charge

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2. Water is a great example of a molecule with polar covalent bonds. How does this bond affect the
Rzqust [24]

Answer :

Example of polar covalent molecules H-O-H(water), ammonia

Explanation:

The presence of intermolecular Hydrogen bonding makes the boiling point of water unexpectedly high, and the polar covalent nature makes it dissolve polar solute/compound

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A reaction that absorbs energy
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Answer:

Endothermic Reaction

Explanation:

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A mixture of 14.2 g of H2 and 36.7 g of Ar is placed in a 100.0 L container at
TiliK225 [7]

a) The total pressure of the system is  1.79 atm

b) The mole fraction and partial pressure of hydrogen is  0.89 and 1.59 atm respectively

c) The mole fraction and the partial pressure  of argon is 0.11 and 0.19 atm.

<h3>What is the total pressure?</h3>

We know tat we can be able to obtain the total pressure in the system by the use of the ideal gas equation. We would have from the equation;

PV = nRT

P = pressure

V = volume

n = Number of moles

R = gas constant

T = temperature

Number of moles of hydrogen = 14.2 g/2g = 7.1 moles

Number of moles of Argon = 36.7 g/40 g/mol

= 0.92 moles

Total number of moles =  7.1 moles + 0.92 moles = 8.02 moles

Then;

P = nRT/V

P = 8.02 * 0.082 * 273/100

P = 1.79 atm

Mole fraction of hydrogen = 7.1/8.02 = 0.89

Partial pressure of hydrogen =  0.89 * 1.79 atm

= 1.59 atm

Mole fraction of argon = 0.92 / 8.02

= 0.11

Partial pressure of argon = 0.11  *  1.79 atm

= 0.19 atm

Learn more about partial pressure:brainly.com/question/13199169

#SPJ1

3 0
1 year ago
1. A gas expands and does p-v work on the surroundings equal to
azamat

The change in energy of the system : -63 J

<h3>Further explanation</h3>

Given

279 J work

216 J heat

Required

The change in energy

Solution

Laws of thermodynamics 1

ΔU=Q+W

Rules :

  • receives heat, Q +  
  • releases heat, Q -  
  • work is done by a system, W -  
  • work is done on a system, W +  

a gas work on the surrounding : W =-279 J

a gas absorb heat from surrounding : Q = +216 J

Internal energy :

= -279+216

= -63 J

3 0
2 years ago
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