(1) A student synthesized Alum and was able to recover a mass of 4.455g of produ

Question

(1) A student synthesized Alum and was able to recover a mass of 4.455g of product. They have calcuated the theoretical yield as 5.668g. calculate the percent yield for this reaction.

(2) calculate the number of moles of KAI(OH)4 that can be made from 0.488 moles of Aluminum foil. (Mwt. Al= 26.98 g/mol) show your work. 2Al(s) + 2KOH(aq) + 6H2O(l) ---> 2KAI(OH)4(aq) + 3H2(g)

(3) 50.0g of acid and 50.0g of base, both at 20.0C, are poured together and the resulting soluble reaches a final temperature of 43.0C. Calculate how much energy (J) was released during the neutralization reaction? (assume no heat lost to environment or calorimeter) E=mC delta T ( C acid and base = 4.184 J/g C )

(4) If 3124J of energy are added to 50.0g of water at 23.0C what temperature would expect the water to reach? (assume no heat loss to environment) E=mC delta T (Cwater = 4.184 J/g C)

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(1) A student synthesized Alum and was able to recover a mass of 4.455g of produ

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