[References] Use the References to access important values if needed for this question. The compound iron (II) acetate, Fe(CH3COO)2 is soluble in water. Write the chemical equation for the dissociation reaction that occurs when solid iron (II) acetate dissolves in water: Be sure to specify states such as (aq) or (s). H₂O

[References] Use the References to access important values if needed for this question. The compound iron (II) acetate, Fe(CH3COO)2 is soluble in water. Write the chemical equation for the dissociation reaction that occurs when solid iron (II) acetate dissolves in water: Be sure to specify states such as (aq) or (s). H₂O

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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G.87.
(LO 4H, 4K, 4N) Classify the type of chemical reaction for Oboth redox and combustion acid-base combustion Ⓒredox combination CH3OH (1) + 2O2(g) → CO₂ (g) + 2H₂O(g)
Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of manganese(II) sulfate and ammonium carbonate are combined. Do not include states such as (s) or (aq). It is not necessarry for you to indicate which of the products is the precipitate.
b) Water "softeners" work via the principle of ion-exchange. The tank of a water softener is filled with a soluble salt such as sodium chloride. As "hard" water passes through the tank, the undesirable ions in hard water (e.g., calcium, magnesium, and iron III) are exchanged for the more desirable "soft" (meaning more soluble) ions like sodium. Explain how swapping the "soft"-water sodium ions for "hard"-water ions would influence the behavior (the cleaning effectiveness) of soaps and detergents.
(c) Cl2(g) + KBr(aq) → KCI(aq) + Br2(g) O combination O decomposition O displacement molecular equation Cl2(g) + reducing agent KBr(aq) KCI(aq) + Br2(g) oxidizing agent total ionic equation | Cl2(g) + CI (aq) + net ionic equation K*(aq) + Br (aq) K+(aq) + Br2(g) Cl2(g) + K+(aq) + Br (aq) → K+(aq) + CI (aq) + | Br2(g)
The reaction A(aq) + B(aq) C(aq) + D(aq) has a ΔHrxn = -85 kJ/mol. This reaction is endorthermic or exothermic . If the temperature of the reaction mixture is increased, equilibrium will shift towards the reactans or products. This change will decrease or increase the concentration of the reactants and K will increase or deacrease
Sodium hydrogen carbonate (NAHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: 圖 HCl(aq) + NaHCO,(aq) → NaCl(aq) + H,O(1) + CO,(g) ol. The CO, gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 250. mL of a 0.065 M HCl solution. What mass of NaHCO, would she need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
Given the following exothermic reaction : Fe3+(aq)+SCN-(aq) <-> FeSCN2+(a1), what will cause the formation of additional FeSCN2+(aq)? Adding heat or Adding Fe(No3)3(aq)? both?
When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: HgO (s) →→→ Hg (1) + 0₂ (g)
Mercury as an amalgam with copper, silver, and tin is used fro fillings in teeth and in the production of chlorine. Soluble mercury compounds can be toxic and must be removed from wastewater. Aqueous mercury (II) nitrate is a toxic compound formed in wastewater and must be removed. To remove this compound, an aqueous sodium sulfide (Na2S) solution is added to wastewater to form a solid mercury (II) sulfide (HgS) precipitate and aqueous sodium nitrate in solution. From the analysis, 0.051 L of 0.010 M mercury (II) nitrate was reacted with 0.020 L of 0.10 M sodium sulfide. Write a balance equation for this chemical reaction. Determine the limiting reactant. How many grams of mercury (II) sulfide form? How many grams of excess reactant remain after the reaction is finished?
Chemistry See page 421 13 Question ... A number of reactions can be used to generate common gases on a laboratory scale. For example, nitrogen can be produced from sodium metal and potassium nitrate as indicated by the balanced equation: 10Na(s) + 2KNO₂ (s)→→→→ K₂O(s) + SNa₂O(s) + N₂(g) A common laboratory-scale reaction can also generate oxygen gas by heating potassium chlorate, as indicated by the balanced equation: 2KCIO3(s) →→→ 2KC1(s) + 30₂(g) ✓ 1st attempt Part 1 What mass of potassium nitrate is needed to generate 177.0 L of gas, composed of 143.0 L of N₂ and 34.0 L of O₂ at 0.920 atm and 299 K, using these two reactions? g KNO, See Hint Part 2 See Hint What mass of potassium chlorate is needed to generate 177.0 L of gas, composed of 143.0 L of N₂ and 34.0 L of O₂ at 0.920 atm and 299 K, using these two reactions? g KCIO
How much water (in mL) should you add to 50.0 mL of 0.300 M H,SO, (ag) to get a solution of 0.130 M H2SO4 (aq)? Write just the numerical answer with proper sig figs (no units) and do not put it in scientific notation. Make sure to record and submit the full work with units and sig figs in the separate file labeled 4 work.