5. Consider the balanced chemical equation 4Al(s)+30,(g)→2A1,O,(s) a. What mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? b. What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely? 6. According to the following balanced equation, calculate the moles of hydrogen produced from 52.6 moles of iron. 3H,SO, (aq)+2Fe(s)→ Fe, (SO,),(aq)+3H,(g) 7. According to the following balanced equation, calculate the mass of needed SİCI4 to produce 3.14 g of HCI. SİCI, (1) +2H,O(1) → SiO,(s)+4HCI(g) 8. Using the unbalanced equation below calculate the theoretical yield of lead (II) carbonate when 1.25 g of lead (II) acetate is treated with carbon dioxide. Pb(C,H,O,), (aq)+H,0(1)+CO,(g)→PbCO,(s)+HC,H,0,(aq) 9. According to his prelab theoretical yield calculations, a student's experiment should have produced 1.44 g of magnesium oxide. When he weighed his product after reaction, only 1.23 g of magnesium oxide was present. What was his percent yield?
5. Consider the balanced chemical equation 4Al(s)+30,(g)→2A1,O,(s) a. What mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? b. What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely? 6. According to the following balanced equation, calculate the moles of hydrogen produced from 52.6 moles of iron. 3H,SO, (aq)+2Fe(s)→ Fe, (SO,),(aq)+3H,(g) 7. According to the following balanced equation, calculate the mass of needed SİCI4 to produce 3.14 g of HCI. SİCI, (1) +2H,O(1) → SiO,(s)+4HCI(g) 8. Using the unbalanced equation below calculate the theoretical yield of lead (II) carbonate when 1.25 g of lead (II) acetate is treated with carbon dioxide. Pb(C,H,O,), (aq)+H,0(1)+CO,(g)→PbCO,(s)+HC,H,0,(aq) 9. According to his prelab theoretical yield calculations, a student's experiment should have produced 1.44 g of magnesium oxide. When he weighed his product after reaction, only 1.23 g of magnesium oxide was present. What was his percent yield?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Can you shown me how to solve 5,6,7,8 and 9
Transcribed Image Text:5. Consider the balanced chemical equation
4Al(s)+30,(g)→2A1,0,(s)
a. What mole ratio would you use to calculate how many moles of oxygen
gas would be needed to react completely with a given number of moles of
aluminum metal?
b. What mole ratio would you use to calculate the number of moles of
product that would be expected if a given number of moles of aluminum
metal reacts completely?
6. According to the following balanced equation, calculate the moles of hydrogen
produced from 52.6 moles of iron.
3H,SO,(aq)+2Fe(s)→ Fe, (SO,),(aq)+3H,(g)
7. According to the following balanced equation, calculate the mass of needed SiCl4
to produce 3.14 g of HCl.
SICI, (1) + 2H,0(1) → SiO,(s) +4HCI(g)
8. Using the unbalanced equation below calculate the theoretical yield of lead (II)
carbonate when 1.25 g of lead (II) acetate is treated with carbon dioxide.
Pb(C,H,O,), (aq)+H,0(1)+CO,(g)→P6CO,(8)+HC,H,O,(aq)
9. According to his prelab theoretical yield calculations, a student's experiment
should have produced 1.44 g of magnesium oxide. When he weighed his product
after reaction, only 1.23 g of magnesium oxide was present. What was his percent
yield?
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