Take the actual sample weight of 13grams, and divide it by the atomic weight of chromium. This gives you your molar percentage of atoms. Now multiply this molar percentage by Avogadro's constant, the number of atoms in one mole, and this will give you your number of atoms in the sample.
86.0 grams Sn (1 mole Sn/118.7 grams)(6.022 X 1023/1 mole Sn)= 4.36 X 1023 atoms of tin=================
1.8x10*24
1 mole = 6.022e23 atoms 8.25 mole = 4.96815 e 24 atoms
A 88,1 gram sample of Ag contain 4,9185.10e23 atoms.
The number of atoms is 1,50553521.10e23.
Quite a few! 147.6 kg chromium (1000 grams/1 kg)(1 mole Cr/52.00 grams)(6.022 X 1023/1 mole Cr) = 1.709 X 1027 atoms of chromium =========================
There are 57.6 grams of tin in that sample.
63.8g
6.022 x 1023= 6.022e+23
341 grams scandium (1 mole Sc/44.96 grams)(6.022 X 1023/1 mole Sc) = 4.57 X 1024 atoms of scandium =====================
2(2+3)=10 atoms 4 chromium atoms and 6 oxygen atoms
The mass of silicon is 4 659 g.
86.0 grams Sn (1 mole Sn/118.7 grams)(6.022 X 1023/1 mole Sn)= 4.36 X 1023 atoms of tin=================
A "mole" of chromium is generally regarded as consisting of Avogadro's Number of atoms. Therefore, 4.37 X 1023 atoms constitutes (4.37 X 1023)/(6.022 X 1023) or 0.726 moles.
Chromium(III) nitrate is not made of molecules. It is ionic. There are 4 ions in one formula of chromium(III) nitrate.
a metal sample weigs 56.8 gramsHow many ounces does this sample weigh?
1.8x10*24