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CHEM 1111 Chapter Notes - Chapter 8: Sulfur Dioxide, Ammonium Chloride, Combustion Analysis

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28 Nov 2016

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Christopher L.Cahill

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Chemical reaction: third hypothesis of john dalton"s theory described it as a process that neither creates nor destroys atoms, it rearranges atoms in chemical compounds, examples: Explosive combination of hydrogen and oxygen gases to produce water: involve changes in energy. Chemical equation: uses chemical symbols to denote what occurs in a chemical reaction. Ammonia and hydrogen chloride react to produce ammonium chloride. Calcium carbonation reactions to produce calcium oxide and carbon dioxide. Equation for process by which sulfur and oxygen react to produce sulfur dioxide. Equation for the reaction of sulfur trioxide and water to produce sulfuric acid. Reactant: each chemical species that appears to the left of the arrow, substances that are consumed in the course of a chemical reaction. Product: each substance that appears to the right of the arrow, substances that form during the course of a chemical reaction.

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Related Questions

Write a balanced equation for the following chemical statements.(Use the lowest possible coefficients.)
(a) A characteristic reaction of Group 1A(1) elements: chunks ofsodium react violently with water to form hydrogen gas and sodiumhydroxide solution.
_____ Na(s) +_____ H2O(l)=_____ H2(g) +______ NaOH(aq)

(b) The destruction of marble statuary by acid rain: aqueous nitricacid reacts with calcium carbonate to form carbon dioxide, water,and aqueous calcium nitrate.
_____ HNO3(aq) + _____ CaCO3(s) = _____CO2(g) +____ H2O(l) +_____Ca(NO3)2(aq)

(c) Halogen compounds exchanging bonding partners: phosphorustrifluoride is prepared by the reaction of phosphorus trichlorideand hydrogen fluoride; hydrogen chloride is the other product. Thereaction involves gases only.
_____PCl3(g) + ____ HF(g) = _____ PF3(g) + ______ HCl(g)

(d) Explosive decomposition of dynamite: liquid nitroglycerine(C3H5N3O9) explodes to produce a mixture of gases - carbon dioxide,water vapor, nitrogen, and oxygen.
_______ C3H5N3O9(l) =___ CO2(g) + ____ H2O(g) + ____ N2(g) + ______O2(g)

Science Tutor: Chemistry Name: Mixtures, Solutions, &Compounds: Chemical Equations Date Chemical Equations If a chemical symbol can be thought of as a letter and a chemical formula as a word in the language of chemistry, then a chemical equation is a statement or sentence. A chemical equation is a shorthand way of describing a chemical reaction between two or more substances. A "+ sign means "combines with." An arrow points away from the reactants and toward the products (See page 10), and an arrow means "yields." 2Na + Cl2 â 2NaCl means sodium combines with chlorine to yield sodiumn chloride (salt) Look closely at the equation above. Notice the "2" in front of NaCI on the right and Na on the left. That 2, called a coefficient, is necessary to make this equation balance. Remember Antoine Lavoisier? (Page 15) Matter is neither created nor destroyed in a chemical reaction. The same number of each kind of atom must be on both sides of a chemical equation. Because chlorine only exists as a molecule consisting of two chlorine atoms, it requires two atoms of sodium to yield two molecules of salt (NaCI). This illustrates another important law stated clearly by the French chemist Joseph-Louis Proust in 1799. Chemical compounds always combine in certain specific fixed proportions. Wherever sodium and chlorine combine, two atoms of sodium will be necessary to react with one molecule of gaseous chlorine. 1 . For the equation 2Mg + O2â 2MgO + energy: A. List the reactant or reactants 2Hato B. List the product or products C. How many atoms of magnesium does it take to combine with one molecule of oxygen? D. How many molecules of magnesium oxide are produced in this reaction? 2. Hydrogen can combine with oxygen to produce water. We could write the equation like this: H2 + O2 â H2O. But this equation is unbalanced! Rewrite this equation with the correct coefficients so that an atom of oxygen doesn't disappear! (Be careful. If you add a coefficient to one side you may have to adjust the other. Count all the atoms.) 3. Now that you have the idea, balance the following equations: A, Pho, â PbO + 02 C. Ca + H2O â Ca(OH)2 + H2 How is following a recipe to mix up a batch of biscuits (or any other food item) similar to Proust's law for chemical reactions? 4. OMark Twain Media, Inc., Publishers 17

097 v 0.79 V 1.12 V 1.00 V 1.59 v .77 V 0.27 V NO *NO, al-NO , a NO -> N,0 , NH, 1.25V 0.9 An arrow represents the "properly balanced reduction half-reaction" between the oxidized species on the left and the reduced species on the right of the arrow. The potential value over each arrow is the standard reduction potential And for that properly balanced half-reaction. For example, from this diagram, you can write NO: (a) + + 2 H(ag) NO2g) + HOI): Ented = +0.79 v (R) (18 pts) When HSEis bubbled into nitric acid solutionss(s), NO(R) NOR)Na(R, and NH (ag) all form. (a) (8 pts) write the four balanced reactions that describe this complex process. (b) (8 pts) For each reaction in part (a), calculate the standard emf (in V. (c) (2 pts) Which of the four reactions has the greatest driving force and which has the least driving force per electron? (2) (16 pts) Use the Latimer diagram above for this question. (a) (6 pts) NOgdisproportionates spontaneously into nitric acid and nitrous acid in acidic media. Show this by writing the balanced chemical reaction and evaluating the standard emf for the reaction. (b) (6 pts) Nitrous acid will not disproportionate spontaneously to nitrogen dioxide and nitric oxide, Show this by writing the balanced chemical reaction and evaluating the standard emf for the reaction. (c) (4 pts) Given that the definition of Ivolt - 1 jouleleoul lomb, show that the reduction of the nitrate ion to nitrogen gas in acidic media has a standard reduction potential of +1.25 v. (3) (6 pts) Active metals like zinc will react with concentrated nitric acid to produce the ammonium ion and the Zn (aq) ion at 25Â°C. (a) (4 pts) write the balanced chemical equation for this process using smallest whole number coefficients. (b) (2 pts) Evaluate AE (V) for the reaction in part (a). (4) (6 pts) Less active metals like copper will react with concentrated nitric acid to produce nitric oxide gas and the Cu *(a) ion at 25Â°C. (Â®) (4 pts) write the balanced chemical equation for this process using smallest whole number coefficients. (b) (2 pts) Evaluate AE for the reaction in part (a). BONUS (8 pts, and PRACTICE): Write all balanced half-reactions indicated by the Latimer diagram above.