How many grams are in #2.3 xx 10^4color(white)(l)"mol"# of calcium phosphate, Ca3(PO4)2?

1 Answer
Feb 22, 2018

#7136900 "g"# or #7136.9 "kg"#

Explanation:

Assuming you mean that we have #2.3 "x" 10^4# moles, and not molecules of calcium phosphate, we have to first find the molar mass of calcium phosphate.

#MW = "Mass of Ca"*3+"Mass of P"*2+"Mass of O"*8#
#MW = 40.1*3+31*2+16*8#
#MW = 310.3 "g"/"mol"#

So now we multiply that number by the number of moles we have:

#2.3 "x" 10^4 "moles" * 310.3 "g"/"mol"#
#2.3 "x" 10^4 color(red)(cancel("moles"))*310.3 "g"/color(red)(cancel("moles"))#
#7136900 "g"# or #7136.9 "kg"#

Hope this helps!