Writing completing chemical equations

Each of the following five procedures results in the formation of a precipitate. For each reaction, write the chemical equations describing the formation of the precipitate the overall equation, the complete ionic equation, and the net ionic equation. Identify the spectator ions. 

STRATEGY Begin by writing the chemical equation for the complete oxidation of octane to carbon dioxide and water. Then calculate the theoretical yield (in grams) of CO, by using the procedure in Toolbox L.l. To avoid rounding errors, do all the numerical work at the end of the calculation. To obtain the percentage yield, divide the actual I mass produced by the theoretical mass of product and multiply by 100%. 

STRATEGY First, we write the chemical equation for the equilibrium and the expression for the solubility product. To evaluate Ksp, we need to know the molarity of each type of ion formed by the salt. We determine the molarities from the molar solubility, the chemical equation for the equilibrium, and the stoichiometric relations between the species. We assume complete dissociation. 

The interhalogen IFT can be made only by indirect routes. For example, xenon difluoride gas can react with iodine gas to produce 1FV and xenon gas. In one experiment xenon difluoride is introduced into a rigid container until a pressure of 3.6 atm is reached. Iodine vapor is then introduced until the total pressure is 7.2 atm. Reaction is then allowed to proceed at constant temperature until completion by solidifying the IF as it is produced. The final pressure in the flask due to the xenon and excess iodine vapor is 6.0 atm. (a) What is the formula of the mterhalogen (b) Write the chemical equation for its formation. 

Rather than write the chemical equation using whole units, a more accurate picture of the reaction is represented by writing the complete ionic equation ... 

STRATEGY As usual, we begin by writing the chemical equation for the solubility equilibrium and the expression for Ksp. The molar solubility is the molarity of formula units in the saturated solution. Because each formula unit produces a known number of cations and anions in solution, we can express the molarities of the cations and anions in terms of s. Then we express Ksp in terms of s and solve for s. Assume complete dissociation. 

Complete the word equations and write balanced chemical equations for the following soluble salt preparations ... 

Step 2 Then write the complete chemical equation for the reaction, using your experience in predicting the formation of a precipitate. 

Writing the chemical equation in the reverse direction requires changing the sign of the cell or half-cell potential. Note that all the equations in Table 17.2 refer to reduction half-reactions, but each complete cell requires one oxidation and one reduction. Thus one of the half-cell equations must be reversed (and the sign of its potential changed) to add to the other to make a complete cell equation. 

You are given the word equation for the reaction between barium nitrate and sodium carbonate. You must determine the chemical formulas and relative amounts of all reactants and products to write the chemical equation. To write the complete ionic equation, you need to show the ionic states of the reactants and products. By crossing out the spectator ions from the complete ionic equation you can write the net ionic equation. The net ionic equation will include fewer substances than the other equations. 

Write the chemical equations for the complete combustion of ethane, ethene, and ethyne into carbon dioxide and water. (Chapter 10)... 

Magnesium hydroxide is a gelatinous material that forms during the water purification process in some water treatment plants because of magnesium ions in the water, (a) Write the chemical equation for the reaction of hydrochloric acid with magnesium hydroxide, (b) Explain what drives this reaction to completion. 

I) Write the chemical equation for the complete oxidation of glucose. 

A sample of 1.50 g of lead(II) nitrate is mixed with 125 mL of 0.100 M sodium sulfate solution, (a) Write the chemical equation for the reaction that occurs, (b) Which is the limiting reactant in the reaction (c) What are the concentrations of all ions that remain in solution after the reaction is complete ... 

A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas at 28 °C and 743 torr pressure, (a) Write balanced chemical equations for the reactions that occur between hydrochloric acid and each component of the mixture, (b) Calculate the total number of moles of carbon dioxide that forms fiom these reactions, (c) Assuming that the reactions are complete, calculate the percentage by mass of magnesium carbonate in the mixture. 

An equation written in this fashion, showing the complete chemical formulas of the reactants and products, is called a molecular equation because it shows tiie chemical formulas of the reactants and products without indicating tiieir ionic character. Because Pb(N03)2, KI, and KNO3 are all soluble ionic compounds and therefore strong electrolytes, we can write the chemical equation to indicate explicitly the ions that are in the solution ... 

X 10 ft of methane at atmospheric pressure and 25°C are oxidized to methanol, (a) What volume of methcmol is formed if the density of CH3OH is 0.791 g/L (b) Write balanced chemical equations for the oxidations of methane and methanol to CO ig) and H20(l). Calculate the total enthalpy change for complete combustion of the... 

For each of the following, write the complete chemical equation for the acid—base reaction that occurs. Describe each using Br0nsted language (if appropriate) and then using Lewis language (show electron-dot formulas). 

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