uets ing for each product whether it is solid (s), liquid (I), aqueous (aq) or gas (g). If no reaction occurs, the products are the same as the reactants, write no reaction and proceed to the next reaction. B. Write an ionic equation for each reaction. Break up only compounds with (aq) into ions. Recall that the number of ions in a compound are indicated with a subscript, but the number of ions listed separately in an equation are indicated with a coefficient. C. Cancel out any ions that appear on both sides of the equation and write the net ionic equation for each. 1. HCl (aq) + Pb(NO3)2 (aq) 2. HCl (aq) + H2SO4 (aq) 3. HCl (aq) + NaHCO3 (aq)

uets ing for each product whether it is solid (s), liquid (I), aqueous (aq) or gas (g). If no reaction occurs, the products are the same as the reactants, write no reaction and proceed to the next reaction. B. Write an ionic equation for each reaction. Break up only compounds with (aq) into ions. Recall that the number of ions in a compound are indicated with a subscript, but the number of ions listed separately in an equation are indicated with a coefficient. C. Cancel out any ions that appear on both sides of the equation and write the net ionic equation for each. 1. HCl (aq) + Pb(NO3)2 (aq) 2. HCl (aq) + H2SO4 (aq) 3. HCl (aq) + NaHCO3 (aq)

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 1STP

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When balancing a chemical equation, which of the following statements is false? l type='a'> Subscripts in the reactants must be conserved in the products. i>Coefficients are used to balance the atoms on both sides. i>The law of conservation of matter must he followed. i>Phases are often shown for each compound hut are not critical to balancing an equation.
List and define all the ways of classifying chemical reactions that have been discussed in the text. Give a balanced chemical equation as an example of each type of reaction, and show clearly how your example fits the definition you have given.
Ammonia can be formed from a combination reaction of its elements. A small fraction of an unreacted mixture of elements is illustrated in the following diagram, in which white spheres represent hydrogen atoms and blue spheres represent nitrogen atoms. The temperature is such that all species are gases. a Write and balance the equation for the reaction. b Which of the following correctly represents the product mixture? c Which species is the limiting reactant? Explain.
Consider the unbalanced equation for the combustion of propane: :math>C3H8(g)+O2(g)CO2(g)+H2O(g) rst, balance the equation. Then, for a given amount of propane, write the mole ratios that would enable you to calculate the number of moles of each product as well as the number of moles of O2that would be involved in a complete reaction. Finally, show how these mole ratios would be applied if 0.55 mole of propane is combusted.
When steel wool (iron) is heated in pure oxygen gas, the steel wool bursts into flame and a fine powder consisting of a mixture of iron oxides ( FeO and Fe2O3 ) forms. Write separate unbalanced equations for the reaction of iron with oxygen to give each of these products.
The Hall process is an important method by which pure aluminum is prepared from its oxide (alumina, Al2O3 ) by indirect reaction with graphite (carbon). Balance the following equation, which is a simplified representation of this process. m:math>Al2O3(s)+C(s)Al(s)+CO2(g)
Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?