Hi, I need help with this problem pls and my teacher is so bad at explaining how to setup the problem and getting the answer for them if you can help me I will appreciate it so much. 5. What is the percent yield when 15.5 g of H2SO4 reacts with excess Al(OH): toproduce 12.8 g of Alb(SO4)3 and water.3 H2SO4 + 2 Al(OH): Al (SO4)3 + 6 H2O(For this problem, you WILL need a stoichiometric setup: MAP the equationabove and use the setup to predict the THEORETICAL YIELD of aluminum sulfatebefore calculating the PERCENT YIELD)

Solution : The percent yield is used to determine the theoretical amount of product percentage…

5. What is the percent yield when 15.5 g of H2SO4 reacts with excess Al(OH): to produce 12.8 g of Ab(SO4)3 and water. 3 H2SO4 + 2 Al(OH): → Al(SO4)3 + 6 H2O (For this problem, you WILL need a stoichiometric setup: MAP the equation above and use the setup to predict the THEORETICAL YIELD of aluminum sulfate before calculating the PERCENT YIELD)

5. What is the percent yield when 15.5 g of H2SO4 reacts with excess Al(OH): to produce 12.8 g of Ab(SO4)3 and water. 3 H2SO4 + 2 Al(OH): → Al(SO4)3 + 6 H2O (For this problem, you WILL need a stoichiometric setup: MAP the equation above and use the setup to predict the THEORETICAL YIELD of aluminum sulfate before calculating the PERCENT YIELD)

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 49A

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