Mole / Molar mass = mass = 0.118 [mol] /169.87 [g mol−1] = 20.05 grams
85 grams of AgNO3 represents 0,.5 moles.
By definition, No. of moles = given mass/molecular mass; and also by definition, molar concentration of a solute means the number of moles of solute per liter of solution. Therefore, 25 mL of 0.068 M AgNO3 contains AgNO3 = (0.068 * 25) / 1000 = 0.0017 mol of AgNO3.The equation for the reaction is AgNO3 + HCl -> AgCl + HNO3, showing that 0.0017 mol of AgNO3 gives 0.0017 mol of AgCl. The molecular mass of AgCl = 107+35.5 = 143.5 gTherefore, the mass of AgCl produced by the reacion = No. of moles*molecular mass = .0017*143.5 = 0.24g, to the justified number of significant digits.100 mL of 0.068 M AgNO3 contains AgNO3 = 0.068 molSo,Therefore,
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
Molarity = moles of solute/liters of solution or, for our purposes moles of solute = liters of solution * Molarity moles of AgNO3 = 0,50 liters * 4.0 M = 2.0 moles of AgNO3 needed --------------------------------------
Roughly 4 moles.
Get moles silver nitrate. 255 grams AgNO3 (1 mole AgNO3/169.91 grams) = 1.5008 moles AgCO3 --------------------------------Now; Molarity = moles of solute/Liters of solution ( 1500 ml = 1.5 Liters ) Molarity = 1.5008 moles AgNO3/1.5 Liters = 1.00 M AgNO3 ---------------------
See it's an easy one..!! AgNO3 + HCl -> AgCl + HNO3 100 mL of 0.068 M AgNO3 contains AgNO3 = 0.068 mol So, 25 mL of 0.068 M AgNO3 contains AgNO3 = (0.068 * 25) / 1000 = 0.0017 mol From the equation, we can see 1 mol of AgNO3 gives 1 mol of AgCl 0.0017 mol of AgNO3 gives 0.0017 mol of AgCl Amount of AgCl can be found this way.! No. of moles = given mass/ molecular mass molecular mass of AgCl = 107+35.5 = 143.5 g Therefore, Given mass = No. of moles*molecular mass = 0.0017*143.5 = 0.244g Note : In your question, you have written 0.068 "m" .. (small) m represents for Molality and (capital) M represents for Molarity..! Hope I helped.. :)
6,2 moles of silver
Divide it by Avogadro constant.There are 0.0088 moles
7.4x10^23 x ( 1 mol AgNO3/ 6.02x10^23) x (169.88g AgNO3/ 1 mol AgNO3)=2.1x10^2g AgNO3no of molecules=7.4x10^23Mr of AgNO3=169.88we can find the no of moles, thereforein 1mol there are 6.02x10^23 molecules7.4x10^23 molecules represent (7.4x10^23/6.02x10^23)molesin theory when we multiply molar mass (Mr) with the no of moles, we obtain the mass of the substance in gram:Mr x no of Mol= Mass in grams(7.4x10^23/6.02x10^23)x169.88= 2.1x10^2
AgNO3 is 169.87 g/mol. Ag is 107.87 g/mol meaning that Ag is 63.5% of AgNO3. 63.5% of 32.46g is 20.61g. 20.61g / 107.87 g/mol = .191 moles.
The number of moles is 0,19.