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How many grams of iron contain 4.06X10^24 atoms of iron?

Sagot :

4.06x20^24/6.02x10^23 = 6.744 moles x 55.845 g/mole = 376.61868grams
okpalawalter8

We have that the grams of iron contained 4.06X10^24 atoms of iron is

g= 376.6g

From the question we are told

How many grams of iron contain 4.06X10^24 atoms of iron?

Generally the equation for the Moles of Iron   is mathematically given as

[tex]M=\frac{4.06x10^24}{6.02x10^23} \\\\M=6.744moles[/tex]

Therefore

Where Molar mass of Iron =55.845

Generally the equation for the mass   is mathematically given as

g= 6.744  x 55.85

g= 376.6g

Therefore

the grams of iron contained 4.06X10^24 atoms of iron is

g= 376.6g

 

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https://brainly.com/question/17756498

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