2. Pure iron reacts with sulfuric acid, H2SO4(9), to form a solutíon of iron sulfate, Fe2(SOs, in water and gaseous hydrogen gas. 3. During photosynthesis in plants, carbon dioxide and water are converted into glucose, CSH1206, and oxygen gas, O,. 4. Acid rain, a solution of sulfurous acid, H.PO(ag), forms when sulfur dioxie Messanger reacts with water. Adrian Cenc

2. Pure iron reacts with sulfuric acid, H2SO4(9), to form a solutíon of iron sulfate, Fe2(SOs, in water and gaseous hydrogen gas. 3. During photosynthesis in plants, carbon dioxide and water are converted into glucose, CSH1206, and oxygen gas, O,. 4. Acid rain, a solution of sulfurous acid, H.PO(ag), forms when sulfur dioxie Messanger reacts with water. Adrian Cenc

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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[Review Topics] [References] "Smelling salts," which are used to revive someone who has fainted, typically contain ammonium carbonate, (NH4)2CO3. Ammonium carbonate decomposes readily to form ammonia, carbon dioxide, and water. The strong odor of the ammonia usually restores consciousness in the person who has fainted. The unbalanced equation is (NH4)2CO3 (8)→ NH3(g) + CO₂(g) + H₂O(g) Calculate the mass of ammonia gas that is produced if 0.850 g of ammonium carbonate decomposes completely. g NH3 Submit Answer Mastered Retry Entire Group 8 more group attempts remaining Previous Next Save and Exit
1. What are the coefficient used to balance the equation below?__Ag2O →__ Ag +___O2a. 2,4,1b. 1,1,1c. 1,4,2d. 2,2,22. Is the following equation balanced? Al + O2 --> 2Al2O3a. trueb. false3. In chemical reactions, what does the principle of conservation of mass mean?a. The total mass of the reactants is less than the total mass of the products.b. Matter is not changed.c. Matter is not created or destroyed.d. The total mass of the reactants is greater than the total mass of the products.4. Is the following equation balanced or unbalanced ? Al + O2 --> Al2O3a. balancedb. unbalanced5. Is the following equation balanced or unbalanced ? N2 +3 H2 --> 2NH3a. balancedb. unbalanced
6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles
65. Balance each of the following equations that describe decomposition reactions. a. CaSO4(s) CaO(s) + SO3 (g) b. Li, CO3 (s) → Li, O(s) + CO2 (9) c. LIHCO3 (s) → Li, CO3 (8) + H2 O(9) + CO2(g) d. C6 H6 (1) → C(s) + H2 (g) e. PB13 (1) → P4(s) + Br2 (1)
9. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following chemical equation: (Be sure to balance the reaction equation) Rh₂(SO4)3(aq) + NaOH(aq) - Rh(OH)³(s) + Na₂SO4(aq) If 69.28 g of rhodium(III) hydroxide is to be produced, what mass of rhodium(III) sulfate will be needed for the reaction?
5. When 5.0 moles of potassium metal reacts with an excess of H₂0, 3.5 g of H2 are produced. 2 K (s) + 2 H20 (1) 2 KOH (aq) H₂ (g) a. Calculate the number of moles of water needed to react with all of the potassium metal. (Ans: 5 mol) + b. Calculate the theoretical yield of H2, in grams, formed when all 5.0 moles of potassium metal are consumed. (Ans: 5.04 g) c. Calculate the percent yield of the reaction, given 3.5 g (actual yield) are produced. (Ans: 69.4%)
The great French chemist Antoine Lavoisier discovered the law of conservation of mass in part by doing a famous experiment in 1775. In this experiment they found that mercury(II) oxide, when heated, decompose into liquid mercury and an invisible and previously unknown substance: oxygen gas. A. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury (II) oxide (HgO) into liquid mercury and gaseous dioxygen. B. Suppose 72 mL of dioxygen gas are produced by this reaction, at a temperature of 120°C and pressure of exactly 1 atm. Calculate the mass of mercury (II) oxide that must have reacted in grams. Round your answer to three significant digits.
Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choices
2KMnO, +5Hg₂Cl₂ + 16HCl→ 10HgCl₂ + 2MnCl₂ + 2KCI+ 8H₂O Using the following data: Reaction: 472.09 1999 Molar mass (g/mol):158.0 Mass (g): 316.1 The excess reactant(s) would be: excess A. Only KMnO₁ B. KMnO, and HCI C. Only HCI D. KMnO, and Hg₂Cl₂ E. KMnO, and HCI
How many grams of Na₂CO3 (molar mass=105.99 g/mol) are formed from the decomposition of 3.75 grams of NaHCO3 molar mass= (84g/mol) according to the following balanced chemical equation. 2NaHCO3+ heat- ---> Na₂CO3 (s) + CO₂(g) + H₂O(g)
Calcium carbonate decomposes to form carbon dioxide and calcium oxide. CaCO3 --> CO2 + CaO. How many liters of carbon dioxide can 200g of CaCO3 generate?