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- 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?hy is the formation of a solid evidence of a chemical reaction? Use a molecular-level drawing in your explanation.The flasks below illustrated three trials of a reaction between varying amounts of zinc and a constant volume of hydrochloric acid solution of constant concentration. The table gives the initial amount of zinc added and the observation at the conclusion of each reaction. Mass of Zinc Added g Observation at Conclusion of Reaction 6.10 Balloon inflated completely Some unreacted zinc remains 2.37 Balloon inflated completely No zinc remains 0.41 Balloon not inflated completely No zinc remains The reaction produces an aqueous solution of zinc chloride and hydrogen gas. Explain the observed results.
- ummarize the simple solubility rules for ionic compounds. How do we use these rules in determining the identity of the solid formed in a precipitation reaction? Give examples including balanced complete and net ionic equations.hy is the formation of a gas evidence of a chemical reaction? Use a molecular-level drawing in your explanation.Using the general solubility rules given in Table 6-1. name three reagents that would form precipitates with each of the following ions in aqueous solution. Write the net ionic equation for each of your suggestions. a. chloride ion b. calcium ion c. iron(III) ion d. sulfate ion e. mercury(I) ion, Hg22+ f. silver ion
- The element tin often occurs in nature as the oxide, SnO2 . To produce pure tin metal from this sort of tin ore, the ore usually is heated with coal (carbon). This produces pure molten tin, with the carbon being removed from the reaction system as the gaseous byproduct carbon monoxide. Write the unbalanced equation for this process.42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.On the basis of the general solubility rules given in Table 4.1, predict the identity of the precipitate that forms when the following aqueous solutions are mixed. If no precipitate forms, indicate which rules apply.
- 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.A common experiment to determine the relative reactivity of metallic elements is to place a pure sample of one metal into an aqueous solution of a compound of another metallic element. If the pure metal you are adding is more reactive than the metallic element in the compound, then the pure metal willreplacethe metallic element in the compound. For example. if you place a piece of pure zinc metal into a solution of copper(II) sulfate, the zinc will slowly dissolve to produce zinc sulfate solution, and the copper(II) ion of the copper(II) sulfate will be converted to metallic copper. Write the unbalanced equation for this process.Apply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.