Answer to Question #180473 in General Chemistry for Yasmine

Question #180473

A chemical reaction takes place and produces 4.75g of product. Stoichiometry predicted a product yield of 5.00g. What is the percent yield of this reaction?




Aluminum reacts with excess copper (II) sulfate according to the unbalanced reaction shown. Balance the equation and indicate the numbers that go in front of each compound. (Give your answer in this format: ___Al + ___CuSO4 → ___Al2(SO4)3 + ___Cu, filling in the blanks.) *





Aluminum reacts with excess copper (II) sulfate according to the unbalanced reaction shown. If 1.85 g of Al react, how many moles of Al reacted? (Give your answer in this format, 0.0xxx mol, with 3 sig. figs.) 







1
Expert's answer
2021-04-13T02:06:56-0400

Percentage yield ="73\\%"


"2Al + 3CuSO_4 \u2192 Al_2(SO_4)_3 + 3Cu"


2.45moles of Al reacted.


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