A pure silver ring contains 2.60X10^22 silver atoms. How many moles of silver atoms it contain?
I did the calculation and I got 4.32 X10^44. Is that correct?
No.
2.60E22/6.022E23 = 0.0432
Did you punch in those numbers on your calculator? The digits are right; the exponent is not. 10^22/10^23 = 10^-1 or 0.1
1 mole is anything is 6.022E23 so
2.60E22 atoms Ag x (1 mol Ag/6.022E23) =?
To find the number of moles of silver atoms in the ring, we can use the Avogadro's number and the given number of silver atoms.
Avogadro's number states that one mole of any substance contains approximately 6.022 x 10^23 particles (atoms, molecules, ions, etc.).
Now, we have the number of silver atoms in the ring, which is 2.60 × 10^22.
To find the number of moles, we divide the number of atoms by Avogadro's number:
Number of moles = Number of atoms / Avogadro's number
Number of moles = 2.60 × 10^22 / 6.022 × 10^23
Now, let's simplify the expression:
Number of moles = (2.60 ÷ 6.022) × (10^22 ÷ 10^23)
Number of moles = 0.431 × 10^(-1)
Number of moles = 0.0431 moles
Therefore, the pure silver ring contains approximately 0.0431 moles of silver atoms.