The amount of moles is also defined as n = m/M, wheren - amount of moles,m - the mass of the substance,M - the atomic mass of the substance (Ag - 107.8682 g/mol), thereforem = n×M = 0.263×107.8682 = 28,369 grams of Ag.
The atomic mass of the element silver, Ag is 108Amount of Ag = mass of sample/molar mass = 108/108 = 1.00 So, there is 1.00mol of silver in a 108g pure sample.
How many moles is in 0.0688 Ag Cl
Oxidation-reduction reaction:Ag^+(aq) + Al(s) ===> Ag(s) + Al^3+ or looked at another way... 3AgNO3(aq) + Al(s) ===> Al(NO3)3(aq) + 3Ag(s) moles AgNO3 present = 92.8 g x 1 mole/170 g =0.546 moles moles Al present = 1.34 g x 1 mole/26.9 g = 0.0498 moles Al is limiting based on mole ratio of 3 AgNO3 : 1 Al moles Ag(s) produced = 0.0498 moles Al x 3 moles Ag/mole Al = 0.1494 moles Ag mass of Ag = 0.1494 moles Ag x 108 g/mole = 16.1 g Ag formed
215.8 g Ag x 1 mol Ag/196.9 = 1.096 moles Ag32.1 g S x 1 mol S/32 g = 1 moles Since Ag and S combine in a ratio of 2:1 (2 Ag to 1 S), the most Ag2S you can form is limited by moles of Ag. 1.096 moles Ag will react with 0.548 moles S ==> Ag2S. So the rest of the S will be left over and not used because there isn't enough Ag. Thus, the mass of resultant salt would be 197 g + 17.5 g = 214.5 g.
The mass of 2,65 Ag moles is 285,85 g.
The amount of moles is also defined as n = m/M, wheren - amount of moles,m - the mass of the substance,M - the atomic mass of the substance (Ag - 107.8682 g/mol), thereforem = n×M = 0.263×107.8682 = 28,369 grams of Ag.
The atomic mass of the element silver, Ag is 108Amount of Ag = mass of sample/molar mass = 108/108 = 1.00 So, there is 1.00mol of silver in a 108g pure sample.
How many moles is in 0.0688 Ag Cl
The equivalent of 68,3 g Ag is 0,633 moles.
The answer is 6,31 moles Ag.
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.
The atomic weight of silver is 107,8682 g/molTo convert grams to moles:moles Ag=35,5 g Ag1 mol= 0,329 mol Ag107,8682 g
Oxidation-reduction reaction:Ag^+(aq) + Al(s) ===> Ag(s) + Al^3+ or looked at another way... 3AgNO3(aq) + Al(s) ===> Al(NO3)3(aq) + 3Ag(s) moles AgNO3 present = 92.8 g x 1 mole/170 g =0.546 moles moles Al present = 1.34 g x 1 mole/26.9 g = 0.0498 moles Al is limiting based on mole ratio of 3 AgNO3 : 1 Al moles Ag(s) produced = 0.0498 moles Al x 3 moles Ag/mole Al = 0.1494 moles Ag mass of Ag = 0.1494 moles Ag x 108 g/mole = 16.1 g Ag formed
215.8 g Ag x 1 mol Ag/196.9 = 1.096 moles Ag32.1 g S x 1 mol S/32 g = 1 moles Since Ag and S combine in a ratio of 2:1 (2 Ag to 1 S), the most Ag2S you can form is limited by moles of Ag. 1.096 moles Ag will react with 0.548 moles S ==> Ag2S. So the rest of the S will be left over and not used because there isn't enough Ag. Thus, the mass of resultant salt would be 197 g + 17.5 g = 214.5 g.
Moles = Mass/ Relative Molecular Mass Aluminum forms Al2 compounds, so the relative molecular mass is 2 * 13 = 26. 856/26 = 32.9 (3sf)
There are 107.9 grams in one mole of pure silver. 107.9 a.m.u. is the average mass of isotopes of the element silver Answer to another (= not this one) question: The atomic number is the number of grams in a mole of any element. Hydrogen has an atomic number of 1 so a mole of hydrogen (okay, a half-mole of H2) weighs 1 gram. [ Silver is not Hydrogen ! and an atom is not a molecule]