3. Write balanced formula equations for each of the following reactions. Physicaistates of reactants and products need not be shown.(i)The combustion of ethane gas, C2H6, in excess air to form carbon dioxideand water.(ii)oxide andcarbon dioxide.The decomposition of solid całcium carbonate by heat to form calcium(iii) The decomposition of hydrogen peroxide to form water and oxygen(iv) Thereaction of iron with chlorine to form iron(III) chloride.

Given (i) Combustion of ethane gas Balance reaction = ? (ii) Decomposition of CaCO3…

Answered: 3. Write balanced formula equations for…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 91QRT

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Please write the balanced chemical equations on the observations of heating NaHCO3 and bubbling the gas made by decomposition through the Ca(OH)2 solution in the presence of bromothymol (blue acid base indicator solution) Please write out in chemical equation form!
Write the reaction quotient, Qc, for each of the following reactions:(a) The first step in nitric acid production, NH3(g) + O2(g) ⇌ NO(g) + H2O(g)(b) The disproportionation of nitrogen monoxide, NO(g) ⇌ N2O(g) + NO2(g)
5. One of the key steps in the tricarboxylic acid (TCA) cycle is the hydration of fumarate to malate: Fumarate-² + H₂O = Malate-2 The standard reaction Gibbs free energy and enthalpy for this reactions are -880 cal/mol and 3560 cal/mol, respectively. (a) What is the equilibrium constant for this reaction (25 °C)? (b) Is the reaction favorable (spontaneous) at 25 °C? (c) What is the equilibrium constant of this reaction under physiological conditions (37 °C)? (d) Is this reaction favorable at 37 °C?
(i) Dry pellets of a base ‘X’ when kept in bpen absorbs moisture and turns sticky. The compound is also formed by chlor-alkali process. Write chemical name and formula of X. Describe chlor-alkali process with balanced chemical equation. Name the type of reaction occurs when X is treated with dilute hydrochloric acid. Write the chemical equation. (ii) While diluting an acid, why is it recommended that the acid should be added to water and not water to the acid?
(a) Halogen, V reacts with hydrogen gas to form HV only when heated to 200 °C in the presence of a platinum catalyst. An aqueous solution of HV is formed when HV is dissolved in water. When aqueous silver nitrate solution is added to the HV solution, precipitate W is formed. With the aid of a balanced chemical equation, explain the reaction between precipitate W and concentrated ammonia solution. () (i) The melting point of hydrogen fluoride, HF is higher than HV. Explain this phenomenon in terms of structure and bonding.
Consider the series of reactions to synthesize the alum (KAl(SO4 )2 · xH2O(s)) from the introduction. (a) Assuming an excess of the other reagents, from one mole of aluminum Al (s), how many moles of alum will be produced? (b) Assuming an excess of the other reagents, from one mole of potassium hydroxide KOH, how many moles of alum will be produced? (c) Assuming an excess of the other reagents, from one mole of sulfuric acid H2SO4 , how many moles of alum will be produced? (d) If you start the synthesis with 1.00 g of Al, 40.0 mL of 1.50 M KOH, and 20.0 mL of 9.00 M H2SO4 , which of the three will be the limiting reagent? (e) Assuming that the product is anhydrous (that there are no waters of hydration), calculate the theoretical yield of alum, in grams, based on the amounts of reagents in part (d). 3. Consider the nickel salt: (NH4 )2Ni(SO4 )2 ·y H2O (Ammonium Nickel Sulfate Hydrate), where y is the number of coordinated waters. (a) Assuming that the product is anhydrous (y = 0),…
Write a balanced equation for each of the followingreactions: (a) Burning magnesium metal in a carbondioxide atmosphere reduces the CO2 to carbon. (b) Inphotosynthesis, solar energy is used to produce glucose(C6H12O6) and O2 from carbon dioxide and water.(c) When carbonate salts dissolve in water, they producebasic solutions.
(a) Write chemical equations to show what happens when each of the following substances is mixed with water: (1) Hydride ion (ii) Glucose, C6H12O6(s) (iii) Copper(II) bromide (iv) Formic acid (b) Write chemical equations for the following processes: 1. Chemical reaction for ΔHf for mercury(I) phosphate 2. Thermal dissociation of gaseous bromine 3. Sublimation of carbon dioxide 4. Reduction of VO2+ to produce VO2+ 5. Neutralization of sulfuric acid by barium hydroxide 6. Themal decomposition of I mol of sodium bicarbonate to produce soditum carbonate, carbon dioxide and water
10. A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process. (a) The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide. (b) The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water. (c) Solid calcium hydroxide is then added to the seawater, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride. (d) The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water. (e) Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorinegas.
The Solvay process for the manufacture of a sodium carbonate begins by passing ammonia and acrbon dioxide through a solution of sodium chloride to make sodium bicarbonate and ammonium chloride. The equation for this reaction is: H2O + NaCl + NH3 + CO2 -> NH4Cl + NaHCO3 In the next step, sodium bicarbonate is heated to give sodium carbonate and two gases, carbon dioxide and steam. 2NaHCO3 -> Na2CO3 + CO2 + H2O 1. What is the theoretical yield of sodium carbonate, expressed in grams, if 164 g of NaCl were used in the first reaction? 2. If 77.9 g of Na2CO3 was obtained, what was the percentage yield?
What are the main equilibria involved in the CO2–Carbonate system and what kind of equilibrium constant is associated with each (K?)?
Please Write the chemical equations for the following processes in the image below.

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