Explanation:
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Answer:
3.59 moles
Explanation:
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The experimental absolute zero value is less when compared to the accepted value of absolute zero.
<h3>What is absolute zero?</h3>
Absolute zero is defined as the temperature in which the lowest energy possible is attained in a thermodynamic system.
Absolute zero temperature has an accepted values of 0 Kelvin or -273.15 degrees Celsius.
At absolute zero, it is assumed that the volume of an ideal gas becomes zero. However, it has not been possible to cool any gas to absolute zero.
Based on the graph of temperature against volume of gases, the experimental absolute zero extrapolated from the graph where volume of the gases becomes zero is -285 degrees Celsius.
Therefore, the experimental absolute zero value is less when compared to the accepted value.
Learn more about absolute zero at: brainly.com/question/1191114
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First a balanced reaction equation must be established:

→

Now if mass of aluminum = 145 g
the moles of aluminum = (MASS) ÷ (MOLAR MASS) = 145 g ÷ 30 g/mol
= 4.83 mols
Now the mole ratio of Al : O₂ based on the equation is 4 : 3
[
4Al +
3 O₂ → 2 Al₂O₃]
∴ if moles of Al = 4.83 moles
then moles of O₂ = (4.83 mol ÷ 4) × 3
=
3.63 mol (to 2 sig. fig.)
Thus it can be concluded that
3.63 moles of oxygen is needed to react completely with 145 g of aluminum.
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