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1. Calculate the percent composition of the first element in the formulas for each of the following compounds. a. CO₂ b. N₂O c. NaOCI

1. Calculate the percent composition of the first element in the formulas for each of the following compounds. a. CO₂ b. N₂O c. NaOCI

Chemistry
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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Hello I was wondering if you could please just provide the answers and no work since in order to receive full credits we must show both the answers and the work but would like to just have an answer key to make sure my work is correct thank you so much have a lovely day :) and I’m sorry that I bothered you
Name Period Date Unit 4 Study Guide Directions: Complete on a separate piece of paper. 1. Calculate the percent composition of the first element in the formulas for each of the following compounds. a. CO₂ bob. N₂O c. NaOCI 2. Give the empirical formula that corresponds to each of the following molecular formulas. a. Na₂O₂ b. CsH6O4 c. C12H12N₂O3 d. C4H6Cl2 3. A compound used in the nuclear industry contains uranium and fluorine. The compound is made up of 67.61% uranium. a. What is percent composition of fluorine? b. What is the empirical formula of the compound? 4. During excessive physical activity, lactic acid (molar mass=90.08 g/mol) forms in muscle tissue and is responsible for muscle soreness. Elemental analysis shows that this compound contains 40% C, 6.71% H, and 53.3% O. a. Determine the empirical formula of lactic acid. b. Determine the molecular formula. 5. Consider the balanced chemical equation 4Al(s)+30₂(g) →2Al₂O₂ (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. 3H₂SO (aq) +2Fe(s)→ Fe₂(SO₂), (aq) + 3H₂(g)
Transcribed Image Text:Name Period Date Unit 4 Study Guide Directions: Complete on a separate piece of paper. 1. Calculate the percent composition of the first element in the formulas for each of the following compounds. a. CO₂ bob. N₂O c. NaOCI 2. Give the empirical formula that corresponds to each of the following molecular formulas. a. Na₂O₂ b. CsH6O4 c. C12H12N₂O3 d. C4H6Cl2 3. A compound used in the nuclear industry contains uranium and fluorine. The compound is made up of 67.61% uranium. a. What is percent composition of fluorine? b. What is the empirical formula of the compound? 4. During excessive physical activity, lactic acid (molar mass=90.08 g/mol) forms in muscle tissue and is responsible for muscle soreness. Elemental analysis shows that this compound contains 40% C, 6.71% H, and 53.3% O. a. Determine the empirical formula of lactic acid. b. Determine the molecular formula. 5. Consider the balanced chemical equation 4Al(s)+30₂(g) →2Al₂O₂ (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. 3H₂SO (aq) +2Fe(s)→ Fe₂(SO₂), (aq) + 3H₂(g)
7. According to the following balanced equation, calculate the mass of needed SiCl4 to produce 3.14 g of HCI. SiCl (1)+2H₂O(1)→SiO₂ (s) + 4HCl(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.co Pb(C₂H₂O₂)₂ (aq) + H₂O(l) + CO₂(g) → PbCO₂ (s) + HC₂H₂O₂(aq) to does not eelur 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? alusstom garwoliot od todos os abogado at slumo) leoniem bavio adTonnoun bus muinsu istabai sun och ai boeu babormos A E
Transcribed Image Text:7. According to the following balanced equation, calculate the mass of needed SiCl4 to produce 3.14 g of HCI. SiCl (1)+2H₂O(1)→SiO₂ (s) + 4HCl(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.co Pb(C₂H₂O₂)₂ (aq) + H₂O(l) + CO₂(g) → PbCO₂ (s) + HC₂H₂O₂(aq) to does not eelur 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? alusstom garwoliot od todos os abogado at slumo) leoniem bavio adTonnoun bus muinsu istabai sun och ai boeu babormos A E
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