Reacting 40.0 mL of 0.200 MAgNO 3 with 40.0 mL of 0.200 MK 2 CrO 4 results in wh
ID: 683420 • Letter: R
Question
Reacting 40.0 mL of 0.200 MAgNO3 with 40.0 mL of 0.200 MK2CrO4 results in what mass of solidformed? a. 0.896 g b. 1.33 g c. 1.79 g d.2.65 g e. none of thesei know the answer is none of these. the actual ancer is 13.3.but i need to know how to get to that answer Reacting 40.0 mL of 0.200 MAgNO3 with 40.0 mL of 0.200 MK2CrO4 results in what mass of solidformed? a. 0.896 g b. 1.33 g c. 1.79 g d.2.65 g e. none of these
i know the answer is none of these. the actual ancer is 13.3.but i need to know how to get to that answer
Explanation / Answer
The number of moles of AgNO3 present = 0.040L*0.200 mol/L = 0.008 mole Similarly the number of moles of K2CrO4 present = 0.040L*0.2mole/L = 0.008 mole The balanced equation of the given reaction is 2AgNO3 +K2CrO4 ---------->Ag2CrO4 (s) + 2KNO3(aq) According to above reaction we conclude that AgNO3 islimiting Therefore mass of the solid formed in the reaction = (0.008 mole AgNO3) ( 1 moleAg2CrO4/ 2 moles ofAgNO3)(331.73g/mole) = 1.326 g of solid is formed. Therefore answer is b)
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