Answer:
For A = 733.2 torr
For B = 740.1 torr
Explanation:
Given data:
For A
Height = 15.4 mm
Pressure of atmosphere = 0.985 atm ( 0.985 ×760 = 748.6 mmHg)
Pressure of gas = ?
For B
Height = 12.3 mm
Pressure of atmosphere = 0.99 atm ( 0.99×760 = 752.4 mmHg)
Pressure of gas = ?
Solution:
For A
P( gas) = P (atmosphere) - 15.4 mmHg
P( gas) = 748.6 mmHg - 15.4 mmHg
P( gas) = 733.2 mmHg or 733.2 torr
For B
P( gas) = P (atmosphere) - 12.3 mmHg
P( gas) = 752.4 mmHg - 12.3 mmHg
P( gas) = 740.1 mmHg
or
740.1 torr
Answer:
See below.
Explanation:
1. Real gases have significant volume.
2. Real gases have more complex interactions than ideal gases.
Atomic radius decreases with the increase of atomic number and mass number because the nuclear charge attracts the outermost shell leads to lower distance of the atom.
<h3>
What is the trend of atomic radius across the periodic table?</h3>
Atomic radius decreases when we go from left to right to a period and increases down a group. In a period, effective nuclear charge increases as electron shielding remains the same. An atom gets larger as the number of orbits or shells increases. The radius of atoms increases as you go down the group in the periodic table. The size of an atom will decrease as you move from left to the right in a period. Within a period, protons are added to the nucleus which attracts electrons closer to the nucleus because of its increased positive charge i.e. proton. So that's why we can say that the force of attraction between nuclei and electrons increases, the atomic radius of the atoms decreases.
So we can conclude that Atomic radius decreases with the increase of atomic number and mass number because the nuclear charge attracts the outermost shell leads to lower distance of the atom.
Learn more about atomic radius here: brainly.com/question/15255548
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