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Determine the number of formula units that are in 0.688 moles of AgNO3?
0.688 moles*6.02x1023=4.14x1023 Formula units
How do you convert 22.6g AgNO3 to moles?
To convert grams to moles, you need to divide the given mass by the molar mass of the substance. The molar mass of AgNO3 is approximately 169.87 g/mol. Therefore, to convert 22.6g of AgNO3 to moles, you would divide 22.6g by 169.87 g/mol to get approximately 0.133 moles of AgNO3.
Silver metal may be precipitated from a solution of silver nitrate by placing a copper strip into the solution. What mass of AgNO3 would you dissolve in water in order to get 1.00 g of silver?
To determine the mass of AgNO3 needed to obtain 1.00 g of silver (Ag), we first need to find the molar mass of silver (approximately 107.87 g/mol) and silver nitrate (AgNO3, approximately 169.87 g/mol). The number of moles of silver in 1.00 g is calculated as ( \frac{1.00 , \text{g}}{107.87 , \text{g/mol}} \approx 0.00926 , \text{mol} ). Since each mole of AgNO3 produces one mole of Ag, the mass of AgNO3 required is ( 0.00926 , \text{mol} \times 169.87 , \text{g/mol} \approx 1.57 , \text{g} ). Therefore, you would need to dissolve approximately 1.57 g of AgNO3 in water to obtain 1.00 g of silver.
Which of the following electrolytes would you use to electroplate silver Ag on iron Fe A. Zn ClO32 B. AgNO3 C. CuCl2 D. FeSO4?
AgNO3
Number of moles and number of atoms in a 214 gram sample of silver?
According to the periodic table, silver (Ag) has an atomic mass of about 108 grams per mole. If you have 802 grams, set up a direct proportion where 108/1=802/x and solve for x. You get about 7.43 moles of silver.
How many moles of silver atoms are in 1.8 x 10 25 atoms of silver?
To calculate the number of moles, you divide the number of atoms by Avogadro's number (6.022 x 10^23). So for 1.8 x 10^25 atoms of silver, the number of moles would be 30 moles.
How many moles of silver nitrate would be required to react with 2.00 moles of sodium phosphate?
I assume double displacement reaction. Balanced equation. 3AgNO3 + Na3PO4 -> Ag3PO4 + 3NaNO3 2.00 moles sodium phosphate ( 3 moles AgNO3/1 mole Na3PO4) = 6.00 moles silver nitrate needed =========================
Determine the number of formula units that are in 0.688 moles of AgNO3?
0.688 moles*6.02x1023=4.14x1023 Formula units
How do you convert 22.6g AgNO3 to moles?
To convert grams to moles, you need to divide the given mass by the molar mass of the substance. The molar mass of AgNO3 is approximately 169.87 g/mol. Therefore, to convert 22.6g of AgNO3 to moles, you would divide 22.6g by 169.87 g/mol to get approximately 0.133 moles of AgNO3.
How many mL of .117M AgNO3 solution would be required to react exactly with 3.82 moles of NaCl?
Balanced equation first! AgNO3 + NaCl -> AgCl + NaNO3 all one to one, get moles AgNO3 3.82 moles NaCl (1 mole AgNO3/1 mole NaCl) = 3.82 moles AgNO3 ------------------------------- Molarity = moles of solute/Liters of solution 0.117 M AgNO3 = 3.82 moles AgNO3/Liters Liters = 3.82/0.117 = 32.6 Liters which is 32600 milliliters which is unreasonable; check answer if you can
A smaple of silver with the same mass as the earth would contain how many atoms of silver and how many moles of silver?
A silver sample with the same mass as the Earth (5.972 × 10^24 kg) would contain about 1.96 × 10^50 atoms of silver. This amount of silver corresponds to approximately 3.25 × 10^25 moles.
Mass of silver in 3.4g AgNO3?
To find the mass of silver in 3.4g of AgNO3, you need to consider the molar mass of silver nitrate (AgNO3). The molar mass of AgNO3 is 169.87 g/mol. Since the molar ratio of Ag to AgNO3 is 1:1, the mass of silver in 3.4g of AgNO3 would be 3.4g * (1/169.87) ≈ 0.02g.
Silver metal may be precipitated from a solution of silver nitrate by placing a copper strip into the solution. What mass of AgNO3 would you dissolve in water in order to get 1.00 g of silver?
To determine the mass of AgNO3 needed to obtain 1.00 g of silver (Ag), we first need to find the molar mass of silver (approximately 107.87 g/mol) and silver nitrate (AgNO3, approximately 169.87 g/mol). The number of moles of silver in 1.00 g is calculated as ( \frac{1.00 , \text{g}}{107.87 , \text{g/mol}} \approx 0.00926 , \text{mol} ). Since each mole of AgNO3 produces one mole of Ag, the mass of AgNO3 required is ( 0.00926 , \text{mol} \times 169.87 , \text{g/mol} \approx 1.57 , \text{g} ). Therefore, you would need to dissolve approximately 1.57 g of AgNO3 in water to obtain 1.00 g of silver.
A sensitive balance can detect masses of 1 10-8 g How many atoms of silver would be in a sample having this mass?
To find the number of atoms in the sample, you would first calculate the number of moles of silver in 1 x 10^-8 g using the molar mass of silver (107.87 g/mol). Then, you would use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms.
Which of the following electrolytes would you use to electroplate silver Ag on iron Fe A. Zn ClO32 B. AgNO3 C. CuCl2 D. FeSO4?
AgNO3
Which of the following electrolytes would you use to electroplate silver (Ag) on iron (Fe)?
agno3
How do you write silver nitrate?
The chemical formula for silver nitrate is AgNO3. To write it, you would denote the symbol "Ag" for silver and "NO3" for the nitrate ion, with the charge balanced to reflect a neutral compound.
