robert7248
07.01.2020 •
Chemistry
Asample of gold (au) has a mass of 35.12 g.
a.
calculate the number of moles of gold (au) in the sample. show your work.
b.
calculate the number of atoms of gold (au) in the sample. show your work
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Ответ:
a. 0.18 mol
b. 1.084 x 10²³ atoms
Explanation:
Data Given:
mass of gold (Au) = 35.12 g
a. number of moles of gold (Au) = ?
b. number of atoms of gold (Au) =?
Solution:
Part a:
To find number of moles following formula will be used
no. of moles = mass in grams / molar mass . . . . . . (1)
molar mass of gold (Au) = 197 g/mol
put values in equation 1
no. of moles = 35.12 g / 197 g/mol
no. of moles = 0.18 mol
so. number of moles of Au = 0.18 mol
Part b:
To find number of atoms following formula will be used
no. of moles = no. of atoms / Avogadro's number
Rearrange the above equation
no. of atoms = no. of moles x Avogadro's number . . . . . . . (2)
Avogadro's number = 6.022 x 10²³ atoms /mol
put values in equation 1
no. of atoms = 0.18 mol x 6.022 x 10²³
no. of atoms = 1.084 x 10²³
so.
number of atoms of Au = 1.084 x 10²³ atoms
Ответ:
Explanation:
Given data:
Mass of gold = 35.12 g
Number of moles of gold = ?
Number of atoms of gold = ?
Solution:
A) Number of moles:
Formula:
Number of moles = mass/ molar mass
Molar mass of gold = 197 g/mol
Number of moles = 35.12 g/ 197 g/mol
Number of moles = 0.18 mol
B) Number of atoms:
The given problem will solve by using Avogadro number.
It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.
The number 6.022 × 10²³ is called Avogadro number .
One mole = 6.022 × 10²³ atoms
0.18 mol × 6.022 × 10²³ atoms / 1mol
1.084 × 10²³ atoms of gold
Ответ:
I do not understand but,
Explanation:
There are 18 groups, 18 columns, and 118 elements at the time of this response.
Here is a map of the periodic table for any more help that you might need.
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