How Many Atoms of Nickel Are Needed to Plate a Steel Part?

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SUMMARY

To determine the number of nickel atoms required to plate a steel part with a surface area of 200 in² and a thickness of 0.002 in, first calculate the volume of nickel needed by multiplying the surface area by the thickness, resulting in 0.4 in³. Next, use the density of nickel, approximately 8.90 g/cm³, to convert the volume into mass. Finally, convert the mass into the number of atoms using Avogadro's number (6.022 x 10²³ atoms/mol) to arrive at the total number of nickel atoms required for plating.

PREREQUISITES
  • Understanding of volume calculation in cubic inches
  • Knowledge of nickel density (8.90 g/cm³)
  • Familiarity with Avogadro's number (6.022 x 10²³ atoms/mol)
  • Basic skills in unit conversion (inches to centimeters, grams to moles)
NEXT STEPS
  • Research the conversion between cubic inches and cubic centimeters
  • Learn about the properties and applications of nickel in plating
  • Study the concept of Avogadro's number and its significance in chemistry
  • Explore density calculations and their relevance in material science
USEFUL FOR

Chemistry students, materials scientists, and engineers involved in metal plating processes will benefit from this discussion.

2slowtogofast
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in order to plate a steel part that has a surface area of 200 in^2 with a 0.002 in thick layer of nickle, how many atoms of nickle are required

not looking for an answer i just need help on what to do. i know how to find how many atoms of somthing when given the weight. just not sure what to do in this case. i was thinking find the volume by 200 * 0.002 then using the density of nickle to find the mass and then go from there. But the numbers i was getting didt seem right.
 
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Your approach looks correct. Can you show us the calculations?
 

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