Respuesta :
Answer:
1 mmol = 1,000 um
[tex]0.80l*\frac{3.2*10^{-5} mmol}{1l}*\frac{1,000um}{1mmol} = 2.6 * 10^{-2} \ um[/tex]
25.6 micromoles when a chemist adds 0.80 L of a 3.2 x [tex]10^{-5}[/tex] mmol/L silver(II) oxide (AgO) solution to a reaction flask.
What are moles?
A mole is defined as 6.02214076 × [tex]10^{23}[/tex]
of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.
The mass of silver nitrate is 0.438 kg
Explanation:
Step 1: Data given
Volume =0.80 L
Molarity silver nitrate (AgO) = 3.2 x [tex]10^{-5}[/tex]M
Molar mass of AgO = 123.868 g/mol
Step 2: Calculate moles AgO
Number of moles = molarity x volume
Number of moles = 3.2 x [tex]10^{-5}[/tex]M x 0.80 L
Number of moles AgO = 2.56×[tex]10^{-5}[/tex] moles
Multiply the number of moles by 1,000,000 to calculate micromoles.
2.56×[tex]10^{-5}[/tex] moles x 1,000,000
25.6 micromoles
Hence, 25.6 micromoles when a chemist adds 0.80 L of a 3.2 x [tex]10^{-5}[/tex] mmol/L silver(II) oxide (AgO) solution to a reaction flask.
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