2 honors chemistry assignment: i need more! gimme more ... · for each question below, write the...
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Assignment: I Need More! Gimme More!Honors Chemistry Unit 07 - Stoichy Page of 1 2
Name: Date:
Task: RecalltheEqua,on: 2H2+O2→2H2O For each question below, write the number of moles of substance beneath its corresponding container. In the third container, draw in the correct number of moles of water produced and any unreacted, excess reactant that is left over. To the right of each question, write the limiting reactant and excess reactant in the space provided.
1)
limiting reactant: __________
excess reactant: __________
________mol H2(g) + ________mol O2(g) → ________mol H2O(g) + ________ mol ________ left over
!
Name: ________________________ Hour: ____ Date: ___________ Chemistry: Visualizing the Limiting Reactant Use the balanced chemical equation 2 H2(g) + O2(g) 2 H2O(g) for all the problems on this sheet. Directions: Assuming that each molecule shown in the first two containers represents one mole of that
substance, write the correct number of moles of substance s below the containers. Then, assume that the contents of the first two containers are combined in the third container. In the third container, draw the correct number of moles of water produced.
1. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) 2. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) In the questions above, all the H2 and O2 reacted. In most reactions, though, the reactants DO NOT combine perfectly; one reactant will be used up before the other; there is too much of one and not enough of the other. The reactant used up first is called the limiting reactant, the other(s) is/are called the excess reactant(s). Directions cont: For each question below, write the number of moles of substances beneath the corresponding containers. In the third container, draw in the correct number of moles of water produced and any unreacted, excess reactant that is left over. To the right of each question, write the limiting and excess reactant. limiting reactant = _______ excess reactant = _______ 3. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 4. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
2)
limiting reactant: __________
excess reactant: __________
________mol H2(g) + ________mol O2(g) → ________mol H2O(g) + ________ mol ________ left over
!
Name: ________________________ Hour: ____ Date: ___________ Chemistry: Visualizing the Limiting Reactant Use the balanced chemical equation 2 H2(g) + O2(g) 2 H2O(g) for all the problems on this sheet. Directions: Assuming that each molecule shown in the first two containers represents one mole of that
substance, write the correct number of moles of substance s below the containers. Then, assume that the contents of the first two containers are combined in the third container. In the third container, draw the correct number of moles of water produced.
1. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) 2. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) In the questions above, all the H2 and O2 reacted. In most reactions, though, the reactants DO NOT combine perfectly; one reactant will be used up before the other; there is too much of one and not enough of the other. The reactant used up first is called the limiting reactant, the other(s) is/are called the excess reactant(s). Directions cont: For each question below, write the number of moles of substances beneath the corresponding containers. In the third container, draw in the correct number of moles of water produced and any unreacted, excess reactant that is left over. To the right of each question, write the limiting and excess reactant. limiting reactant = _______ excess reactant = _______ 3. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 4. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
3)
limiting reactant: __________
excess reactant: __________
________mol H2(g) + ________mol O2(g) → ________mol H2O(g) + ________ mol ________ left over
!
Name: ________________________ Hour: ____ Date: ___________ Chemistry: Visualizing the Limiting Reactant Use the balanced chemical equation 2 H2(g) + O2(g) 2 H2O(g) for all the problems on this sheet. Directions: Assuming that each molecule shown in the first two containers represents one mole of that
substance, write the correct number of moles of substance s below the containers. Then, assume that the contents of the first two containers are combined in the third container. In the third container, draw the correct number of moles of water produced.
1. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) 2. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) In the questions above, all the H2 and O2 reacted. In most reactions, though, the reactants DO NOT combine perfectly; one reactant will be used up before the other; there is too much of one and not enough of the other. The reactant used up first is called the limiting reactant, the other(s) is/are called the excess reactant(s). Directions cont: For each question below, write the number of moles of substances beneath the corresponding containers. In the third container, draw in the correct number of moles of water produced and any unreacted, excess reactant that is left over. To the right of each question, write the limiting and excess reactant. limiting reactant = _______ excess reactant = _______ 3. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 4. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
4)
limiting reactant: __________
excess reactant: __________
________mol H2(g) + ________mol O2(g) → ________mol H2O(g) + ________ mol ________ left over
!
Name: ________________________ Hour: ____ Date: ___________ Chemistry: Visualizing the Limiting Reactant Use the balanced chemical equation 2 H2(g) + O2(g) 2 H2O(g) for all the problems on this sheet. Directions: Assuming that each molecule shown in the first two containers represents one mole of that
substance, write the correct number of moles of substance s below the containers. Then, assume that the contents of the first two containers are combined in the third container. In the third container, draw the correct number of moles of water produced.
1. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) 2. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) In the questions above, all the H2 and O2 reacted. In most reactions, though, the reactants DO NOT combine perfectly; one reactant will be used up before the other; there is too much of one and not enough of the other. The reactant used up first is called the limiting reactant, the other(s) is/are called the excess reactant(s). Directions cont: For each question below, write the number of moles of substances beneath the corresponding containers. In the third container, draw in the correct number of moles of water produced and any unreacted, excess reactant that is left over. To the right of each question, write the limiting and excess reactant. limiting reactant = _______ excess reactant = _______ 3. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 4. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
!
limiting reactant = _______
excess reactant = _______ 5. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 6. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 7. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 8. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 9. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over limiting reactant = _______ excess reactant = _______ 10. _____ mol H2(g) _____ mol O2(g) _____ mol H2O(g) + _____ mol _____ left over
Revised 2017-2018 Honors Chemistry
Assignment: I Need More! Gimme More!Honors Chemistry Unit 07 - Stoichy Page of 2 2
5. How do you know you have a “limiting reactant” problem?
6. Develop and record a strategy for solving “limiting reactant” problems. What do you do first?
7. Use your strategy to solve the following “limiting reactant” problem. Then reflect on your strategy and adjust it to fit your working knowledge. You have 0.750mol of aluminum oxide and 2.50mol of water. Write the balanced chemical equation for the syn-thesis reaction that occurs when these two substances react. How many moles of aluminum hydroxide is pro-duced? Which reactant is limiting? Which reactant is in excess? How many moles of excess reactant is left over?
Revised 2017-2018 Honors Chemistry