Use the equation below to answer the following questions.
Al + H2SO4 ==> Al2(SO4)3 + H2
A. If 8.15 moles of aluminum are reacted, how many moles of hydrogen will be produced?
B. If 44.7 g of hydrogen sulfate is reacted, what mass of aluminum sulfate is produced?
C. If 34.6 g of hydrogen sulfate is reacted, how many moles of aluminum is also reacted?
D. What mass of aluminum is needed to produce 0.321 moles of hydrogen?
You need to balance the equation.
2Al + 3H2SO4 ==> Al2(SO4)3 + 3H2
Now use the coefficients to convert mols Al to mols H2.
mols H2 = mols Al x (3 mols H2/2 mols Al) = ??
Note how the mols Al cancel to leave mols H2. That is how you know if the conversion factor you are using is the right one (instead of using 2 mols Al/3 mols H2.
To answer these questions, we need to use the balanced chemical equation provided.
The equation is: Al + H2SO4 → Al2(SO4)3 + H2
A. To find the number of moles of hydrogen produced when 8.15 moles of aluminum is reacted, we can use the mole ratio from the balanced equation. According to the equation, the mole ratio of aluminum to hydrogen is 1:1. Therefore, the number of moles of hydrogen produced will also be 8.15 moles.
B. To find the mass of aluminum sulfate produced when 44.7 g of hydrogen sulfate reacts, we need to use the molar mass and stoichiometry. First, calculate the number of moles of hydrogen sulfate using its molar mass. Then, use the mole ratio of aluminum sulfate to hydrogen sulfate, which is 1:1, to determine the number of moles of aluminum sulfate produced. Finally, multiply the number of moles of aluminum sulfate by its molar mass to find the mass in grams.
C. To determine the number of moles of aluminum that reacts with 34.6 g of hydrogen sulfate, we follow the same steps as in question B. First, calculate the number of moles of hydrogen sulfate using its molar mass. Then, use the mole ratio of aluminum to hydrogen sulfate, which is 1:1, to determine the number of moles of aluminum that reacts.
D. To find the mass of aluminum needed to produce 0.321 moles of hydrogen, we need to use the molar mass and stoichiometry. First, use the mole ratio of aluminum to hydrogen, which is 1:1, to determine the number of moles of aluminum required. Then, multiply the number of moles of aluminum by its molar mass to find the mass in grams.
Remember to always use the balanced chemical equation, mole ratios, and molar masses when solving stoichiometry problems like these.