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Q: How many moles are in 0.525g of AgCl?
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How many moles is 573.28g of AgCl?

There's 4 moles.


How many moles is 573.28 g of AgCl?

Remember the equation moles = mass(g) / Mr Mr is the relative molecular mass. Refer to the Periodic Table 1 x Ag = 1 x 107.87 1 x Cl = 1 x 35.5 107.87 + 35.5 = 143.37 (Mr of AgCl) Substituting moles(AgCl) = 573.28 / 143.37 = 3.9986... ~ 4 moles (AgCl)


How many moles of silver chloride are produced from 7 moles of silver nitrate?

AgNO3 + NaCl ===> AgCl(s) + NaNO37 moles silver nitrate will produce 7 moles of silver chloride provided there is sufficient (at least 7 moles) of sodium chloride.


An impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgNO3 formed 2.044 g of Ag-Cl what is the percentage of Na-Cl in the impure sample?

2.044 g AgCl / 143.33 g per mole = 0.01426 moles of AgClNaCl + AgNO3 --> AgCl + NaNO31 mole of AgCl = 1 mole of NaClThe sample contained 0.01426 moles of NaCl0.01426 moles NaCl x 58.44 g per mole = 0.8334 g NaCl0.8334 / 0.8421 = 98.97% pureI'm pretty sure this is the correct answer.


What mass of solid agcl is obtained when 25 ml of 0.068m agno3 reacts with excess of aqueous hcl?

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,

Related questions

How many moles is 573.28g of AgCl?

There's 4 moles.


How many moles of AgCl will be produced from 83.0 g of AgNO3 assuming NaCl is available in excess?

X = 0.489 moles of AgCl produced


How many moles is 573.28 g of AgCl?

Remember the equation moles = mass(g) / Mr Mr is the relative molecular mass. Refer to the Periodic Table 1 x Ag = 1 x 107.87 1 x Cl = 1 x 35.5 107.87 + 35.5 = 143.37 (Mr of AgCl) Substituting moles(AgCl) = 573.28 / 143.37 = 3.9986... ~ 4 moles (AgCl)


How many moles of silver chloride are produced from 7 moles of silver nitrate?

AgNO3 + NaCl ===> AgCl(s) + NaNO37 moles silver nitrate will produce 7 moles of silver chloride provided there is sufficient (at least 7 moles) of sodium chloride.


Do chemical reactions contain the same number of moles as reaction proceeds?

Not necessarily. Some reactions do have the same number of moles, and some do not.Examples: NaCl + AgNO3 ==> NaNO3 + AgCl same # of moles N2 + 3H2 ==> 2NH3 different # of moles


An impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgNO3 formed 2.044 g of Ag-Cl what is the percentage of Na-Cl in the impure sample?

2.044 g AgCl / 143.33 g per mole = 0.01426 moles of AgClNaCl + AgNO3 --> AgCl + NaNO31 mole of AgCl = 1 mole of NaClThe sample contained 0.01426 moles of NaCl0.01426 moles NaCl x 58.44 g per mole = 0.8334 g NaCl0.8334 / 0.8421 = 98.97% pureI'm pretty sure this is the correct answer.


What mass of solid agcl is obtained when 25 ml of 0.068m agno3 reacts with excess of aqueous hcl?

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,


How many grams of solid AgCl are needed to make 4.0 liters of a 5.0 M solution of AgCl?

newtest3


How many atoms in AgCl?

A formula unit of AgCl contains 2 atoms: 1 of silver and 1 of chlorine.


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


Is AgCl soluble?

AgCl is relatively insoluble.


What mass of silver chloride in grams will precipitate when 100 mL of 0.100 M hydrochloric acid is added to 68.8 mL of 0.100 M silver nitrate solution?

First, find how many moles in each reagent.As a rule, Molarity (M) = number of moles/volume of solution in litersthen, number of moles = Molarity (M) x volume of solution in litresSo, number of moles of hydrochloric acid = 0.100 x 0.100 = 0.01 molesand number of moles of silver nitrate solution = 0.100 x 0.688 = 0.0688 molesAs the amount of silver nitrate is in excess, then hydrochloric acid is the limiting reagent, which means that the maximum amount of silver chloride can be obtained when all the 0.01 moles of hydrochloric acid react.Now, let us get the balanced equation for the reaction:AgNO3(aq) + HCl(aq) = AgCl(s) + HNO3(aq)It's clear from the above equation that the ratio of HCl : AgCl is 1:1Meaning that if you react 0.01 moles of HCl with AgNO3 you will be getting 0.01 mole of AgCl.Now, check your university periodic table for proper values of RAMs of each of Ag and Cl (mine are 108 and 35.5 respectively)Therefore, the maximum amount of AgCl that can be obtained from this reaction is 0.01 x (108 + 35.5) = 1.435g of AgCl