Consider the equation of aluminum with sulfuric acid as shown below: 2Al (s) + 3H2SO4 (aq) ⟶ Al2(SO4)3 (aq) + 3H2 (g) a) Classify the reaction. b) How many moles of H2SO4 are required to completely react with 6.90 mole Al? c) How many grams of H2 gas will be formed if 4.75 grams of aluminum reacts with excess sulfuric acid?
Consider the equation of aluminum with sulfuric acid as shown below:
2Al (s) + 3H2SO4 (aq) ⟶ Al2(SO4)3 (aq) + 3H2 (g)
a) Classify the reaction.
b) How many moles of H2SO4 are required to completely react with 6.90 mole Al?
c) How many grams of H2 gas will be formed if 4.75 grams of aluminum reacts with excess sulfuric acid?
d) If we begin with 275 grams of aluminum and 275 grams of sulfuric acid, what would be the aluminum sulfate theoretical yield of the reaction?
e) Calculate number of molecules of aluminum sulfate from the theoretical yield obtained from part d).
Use units, significant figures correctly. For very large or small numbers, be sure to express responses in scientific notation. Show your work neatly.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
