Given the reaction:ferrous oxidealuminum25.0g ferrous oxide reacts with 5.0g aluminum5. Which of the following is the correct chemical equation for the given reaction?A. Fe₂O3AlFe+B. FeOAlFe+Fe+Fe+6.8.C. Fe₂OD. FeO₂9.7. Which is the limiting reactant?A ferrous oxideB. aluminum+++A.B.AlAlHow many moles of the excess reagent will be left?0.9230.463When the above equation is correctly balanced using smallest whole number coefficients, the sum of all thecoefficient isA. 10B. 5iron +How many grams of iron will be formed?A. 23.6gB. 70.8gAl₂O3Al₂O3Al3O2Al₂O3aluminum oxideC. 9D. 7с.ironD. aluminum oxideC. 12.5D. 0.0695C. 15.56gD. 35.4g

Answered: Image /qna-images/answer/27cc054e-4c48-451d-a9ed-4fd868aeeced.jpg

Given the reaction: ferrous oxide aluminum 25.0g ferrous oxide reacts with 5.0g aluminum 5. Which of the following is the correct chemical equation for the given reaction? A. Fe₂O3 Al Fe + B. FeO Fe + C. Fe₂O + D. FeO₂ + + + + A. 10 B. 5 Al Al Al 7. Which is the limiting reactant? A ferrous oxide B. aluminum Fe Fe 6. When the above equation is correctly balanced using smallest whole number coefficients, the sum of all the coefficient is 8. How many moles of the excess reagent will be left? A. 0.923 B. 0.463 9. How many grams of iron will be formed? A. 23.6g B. 70.8g iron + Al₂O3 Al₂O3 Al3O₂ Al₂O3 aluminum oxide C. 9 D. 7 C. iron D. aluminum oxide C. 12.5 D. 0.0695 C. 15.56g D. 35.4g

Given the reaction: ferrous oxide aluminum 25.0g ferrous oxide reacts with 5.0g aluminum 5. Which of the following is the correct chemical equation for the given reaction? A. Fe₂O3 Al Fe + B. FeO Fe + C. Fe₂O + D. FeO₂ + + + + A. 10 B. 5 Al Al Al 7. Which is the limiting reactant? A ferrous oxide B. aluminum Fe Fe 6. When the above equation is correctly balanced using smallest whole number coefficients, the sum of all the coefficient is 8. How many moles of the excess reagent will be left? A. 0.923 B. 0.463 9. How many grams of iron will be formed? A. 23.6g B. 70.8g iron + Al₂O3 Al₂O3 Al3O₂ Al₂O3 aluminum oxide C. 9 D. 7 C. iron D. aluminum oxide C. 12.5 D. 0.0695 C. 15.56g D. 35.4g

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...

See similar textbooks

Similar questions

Using the balanced equation, 2 NO + O 2------> 2 NO 2, deter mine the limiting reactant under each of the following conditions. a. 1.0 mol NO and 1.0 mol O 2 c. 10.0 g NO and 10.0 g O 2 b. 2.0 mol NO and 0.50 mol O 2 d. 28.0 g NO and 16.0 g O 2
Balance the following chemical equations: 1. The reaction between iron and oxygen in the air produces rust. Fe+0 Fe O 2. Car engine burns fuel. Combustion or burning takes place when methane combines with oxygen in the air to produce carbon dioxide and water vapor. +0. Aco+HO 16 Hyperacidity is observed when the stomach becomes too acidic. Antacids such as calcium hydroxide are used to neutralize the hydrochloric acid inside the stomach. 3. Ca(OH) + HCI CaCl +H.0
Consider the generic chemical equation: 2 A + 4 B --------> 3 C 1. If 10.0 moles of each reactant were used to complete that reaction, which of the following is true. a. A is the limiting reactant and 15.0 moles of C will be produced. b. A is the limiting reactant and 20.0 moles of C will be produced. c. B is the limiting reactant and 7.50 moles of C will be produced. d. B is the limiting reactant and 22.5 moles of C will be produced. 2. What is the percent yield of this reaction if 6.40 moles of C were actually produced?
Iron oxide reacts with carbon to produce elemental iron and carbon monoxide according the the equation shown below. Consider the reaction of 51.4 grams of Fe2O3 with 24.98 grams of C to produce 19.20 grams of Fe. Fe2O3(s)+3c(s)-------2Fe(s)+3CO(g) a. actual yield b. theoretical yield c. percent yield
Please answer all parts of this question. 1. Magnesium oxide can be made by heating magnesium metal in the presence of oxygen gas. a. Write the balanced equation, including phase symbols. b. When 10.1 g of magnesium reacts with 10.5 g of oxygen gas, 11.9g of magnesium oxide is collected. i. Determine the limiting reactant ii. Determine the theoretical yield iii. Determine the percent yield for the reaction
3. Phosphorus trichloride reacts with water to form phosphorous acid, H3PO3, and hydrochloric acid in the following unbalanced reaction. What is the coefficient of PCI3 in the balance reaction? PCI3 + H2O → H3PO3 + HCI а. 1 b. 3 С. 2 d. 4
Which of the following represents the correct balanced chemical equation for the burning of coal which is still a major source of electricity in the United States. A. C + O --> CO B. C + O2 --> CO2 C. C (s) + O (g) --> CO2 (g) D. C (s) + O2 (g) --> CO2 (g)
DONE 5. The reaction shown below is balanced, use it to answer the following questions. 4Fe(s) + 302(g) 2Fe2O3(s) a. If 4 Fe are used for every 302, how many moles of Fe203 are formed? 2 mols of Fe203 form b. Determine 3 different mole ratios of reactants and products using the balanced equation. c. If you start with 9.100 g Fe and an unlimited amount of O2 from the air, how many grams of Fe203 will be formed? d. If you start with 2.75 moles of Fe and an unlimited amount of O2, how many grams of I They A G The & 7 8
1. What coefficients (in order from left to right) are needed to balance the following chemical equation? ___Fe2O3(s) + ___C(s) → ___Fe(s) + ___CO(g) a. 1, 2, 3, 3 b.1, 2, 1, 3 c 1, 3, 2, 3 d.2, 1, 2, 3
3. Consider the following balanced reaction: 2 Fe + 3 Cl₂ → 2 FeCl3 Given 60.0 g of Fe and excess Cl₂ (as much as we need), calculate: a. The theoretical yield of FeCl3, in grams. b. The theoretical amount of Cl₂ consumed, in grams.
4. C3H8 +O2 _CO2 +_H20 a. Balance the reaction b. What is the reaction type? c. What is the theoretical volume (L) of carbon dioxide produced from the reaction of 20.3L of propane? d. If 58.2L of CO2 is actually produced, what is the percent yield? e. What is the percent error?
15. Titanium (IV) chloride is reduced by magnesium to produce titanium according to the following reaction. a. TiCla(s) + 2Mg(s) → Ti(s) + 2MgCl2(s) How many grams of TiCla(s) can be reduced to Ti by 2000.0g of Mg?