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1020g
The balanced reaction is this:(NH4)CO3 + Ag2SO4 ---> Ag2CO3 + (NH4)2SO4To solve this:1) convert the 10.0 grams of (NH4)CO3 into moles (see Related Questions)2) determine the stoichiometry of the reaction to determine how many moles of Ag2CO3 are produced (see Related Questions)3) because there is an excess of Ag2SO4 , the number of moles of (NH4)CO3 will determine the number of moles of Ag2CO34) convert the number of moles of Ag2CO3 into grams (see Related Questions)
None, unless there is metallic potassium in the reaction mixture. Assuming excess potassium metal is present then 14 moles of KBr can be produced. 7BaBr2 + excess potassium -----> 14KBr + 7 Ba
30 moles
4 moles
Also 5,8 mol
1020g
0.125 Molar solution! Molarity = moles of solute/Liters of solution Algebraically manipulated, Moles of copper sulfate = 2.50 Liters * 0.125 M = 0.313 moles copper sulfate needed ===========================
6 moles
hahaha cheating with a website, how cliche. answer is .28 moles..enjoy
hahaha cheating with a website, how cliche. answer is .28 moles..enjoy
The balanced reaction is this:(NH4)CO3 + Ag2SO4 ---> Ag2CO3 + (NH4)2SO4To solve this:1) convert the 10.0 grams of (NH4)CO3 into moles (see Related Questions)2) determine the stoichiometry of the reaction to determine how many moles of Ag2CO3 are produced (see Related Questions)3) because there is an excess of Ag2SO4 , the number of moles of (NH4)CO3 will determine the number of moles of Ag2CO34) convert the number of moles of Ag2CO3 into grams (see Related Questions)
X = 0.489 moles of AgCl produced
30 moles
None, unless there is metallic potassium in the reaction mixture. Assuming excess potassium metal is present then 14 moles of KBr can be produced. 7BaBr2 + excess potassium -----> 14KBr + 7 Ba
4 moles
4 moles