There are 12.052 ×10²³ atoms in 54 g of aluminium according to the concept of Avogadro's number.
Avogadro's number is defined as a proportionality factor which relates number of constituent particles with the amount of substance which is present in the sample.
It has a SI unit of reciprocal mole whose numeric value is expressed in reciprocal mole which is a dimensionless number and is called as Avogadro's constant.It relates the volume of a substance with it's average volume occupied by one of it's particles .
According to the definitions, Avogadro's number depend on determined value of mass of one atom of those elements.It bridges the gap between macroscopic and microscopic world by relating amount of substance with number of particles.
Number of atoms can be calculated using Avogadro's number as follows: mass/molar mass×Avogadro's number
Substituting the values in the formula,54/26.98×6.022×10²³=12.052×10²³ atoms .
Hence, there are 12.052×10²³ atoms in 54 g of aluminium.
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to the nearest hundredth?
Grams are the unit of the mass that is used to calculate the moles. From 37.5 gms of iron, 53.6 gms of ferric oxide are produced.
Mass is the measurement of the moles of the substance and the molar mass.
Moles of iron from the mass is calculated as:
Moles of iron = 37.5 gms ÷ 55.84 = 0.671 moles
The balanced chemical reaction:
4Fe + 3O2 → 2Fe2O3
From the above it is deduced that 4 moles of iron produce 2 moles of ferric oxide so, 0.671 moles of iron will produce,
(0.671 × 2) ÷ 4 = 0.3375 moles
Mass of ferric oxide, from moles, is calculated as:
Mass = 0.33 moles × 159.687
= 52.696 gms
Therefore, 53.6 gms of ferric oxide will be produced from 37.5 gms of iron.
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The mass of Fe2O3 that can be produced from 37.5g of iron (Fe) is approximately 53.65g. This is achieved by converting mass of iron to moles, using stoichiometry from the balanced chemical equation to convert moles of iron to moles of Fe2O3, and then converting moles of Fe2O3 back to grams.
First, we need to figure out the molar mass of iron (Fe) which is approximately 55.85 g/mol and the molar mass of iron(III) oxide (Fe2O3) which is approximately 159.69 g/mol. We find this using the atomic masses of Iron (Fe) and Oxygen (O) from the periodic table and add them appropriately.
Next, to find the number of moles of iron we use the provided mass of Fe and its molar mass. We calculate this as (37.5 g Fe / 55.85 g/mol Fe) = 0.671 moles of Fe. Now, the balanced chemical equation for the formation of iron(III) oxide is: 4Fe + 3O2 --> 2Fe2O3. From this balanced equation, we know that it takes 4 moles of iron (Fe) to produce 2 moles of Fe2O3. Therefore, the moles of Fe2O3 formed from 0.671 moles of Fe would be (0.671 moles Fe * 2 moles Fe2O3/4 moles Fe) = 0.336 moles of Fe2O3.
Finally, to find the mass of Fe2O3 produced, we multiply the moles of Fe2O3 by its molar mass. We calculate this as (0.336 moles Fe2O3 * 159.69 g/mol Fe2O3) = 53.657 g of Fe2O3.
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B amount of matter in a substance
c feree times distance-
D distance divided by the time
Answer:
a
Explanation:
ability to cause change in matter or the capacity to do work