The average atomic mass of element X is 10.025 amu
The average atomic mass of element X = atomic mass of 10 isotope × relative abundance of 10 isotope + atomic mass of 11 isotope × relative abundance of 11 isotope + atomic mass of 12 isotope × relative abundance of 12 isotope
= 10 × 98% + 11 × 1.5 % + 12 × 0.5 %
= 10 × 0.98 + 11 × 0.015 + 12 × 0.005
= 9.8 + 0.165 + 0.06
= 10.025 amu
So, the average atomic mass of element X is 10.025 amu
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The concept of resonance is required for certain molecules because the localized electron model assumes electrons are located between a given pair of atoms in a molecule.
They will stay the same through the laws of conservation of mass even when they have changed state so they will have the reactant of Ice will be the same amount as the product of water
Answer:
V = 22.42 L/mol
N₂ and H₂ Same molar Volume at STP
Explanation:
Data Given:
molar volume of N₂ at STP = 22.42 L/mol
Calculation of molar volume of N₂ at STP = ?
Comparison of molar volume of H₂ and N₂ = ?
Solution:
Molar Volume of Gas:
The volume occupied by 1 mole of any gas at standard temperature and pressure and it is always equal to 22.42 L/ mol
Molar volume can be calculated by using ideal gas formula
PV = nRT
Rearrange the equation for Volume
V = nRT / P . . . . . . . . . (1)
where
P = pressure
V = Volume
T= Temperature
n = Number of moles
R = ideal gas constant
Standard values
P = 1 atm
T = 273 K
n = 1 mole
R = 0.08206 L.atm / mol. K
Now put the value in formula (1) to calculate volume for 1 mole of N₂
V = 1 x 273 K x 0.08206 L.atm / mol. K / 1 atm
V = 22.42 L/mol
Now if we look for the above calculation it will be the same for H₂ or any gas. so if we compare the molar volume of 1 mole N₂ and H₂ it will be the same at STP.
Answer:
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Explanation:
