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More information about this seller Contact this seller. Brand new. Seller Inventory SKU Student ed. Language: English. Brand new Book. Seller Inventory AAC Brand New!. How do the boiling points of the group 4A hydrides change as the molecular masses of the hydrides change? What are the molecular structure and polarity of the four group 4A hydrides? Predict the strength of the forces between group 4A hydride molecules. Explain how those forces affect the boiling points of group 4A hydrides.
How do the boiling points of the group 6A hydrides change as the molecular masses of the hydrides change? What are the molecular structure and polarity of the four group 6A hydrides? Use Table in your textbook to determine the difference in electronegativities of the bonds in the four group 6A hydrides.
Chemistry matter and change chapter 16 chapter assessment
Answer the following questions about the simple mercury barometer shown here. Use with Chapter 14, Section At sea level At meters above sea level Figure 1 Figure 2 2. What prevents mercury from flowing out of the glass tube into the bowl of mercury? When the barometer in Figure 1 is moved to a higher elevation, such as an altitude of 4.
Suppose the barometer in Figure 1 was carried into an open mine meters below sea level. How would the height of the mercury column change? Explain why. Suppose the liquid used to make the barometer was water instead of mercury. How would this substitution affect the barometer? How would this event affect the column of mercury? Why is the mercury column lower in Figure 2 than in Figure 1? Answer the following questions about this solution. Why do the sugar molecules in the solution lower the vapor pressure of the water? What is the number of moles of sucrose in the solution?
What is the number of moles of water in the solution? What is the mole fraction of water in the solution? How much is the vapor pressure of the solution reduced from that of water by the addition of the sucrose? Use this diagram to help you answer the questions below about the second diagram.
Use with Chapter 16, Section On the diagram at the right, draw arrowheads to show the directions in which the three lines labeled 1, 2, and 3 should point. Enthalpy 3. Answer the following questions about the reaction. What is the concentration of N2O5 at the beginning of the experiment? After 1 hour? After 2 hours? After 10 hours? Calculate the percentage of change the concentration undergoes during the first hour of the reaction. What is the instantaneous rate of reaction for the decomposition of N2O5 for the time period between the first and second hours of the reaction?
Between the second and third hours?
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Between the sixth and seventh hours? What is the instantaneous rate of reaction for the decomposition of N2O5 between the sec- ond and fourth hours of the reaction? Between the third and eighth hours of the reaction? How long does it take for 0. What is the average rate of reaction for the decomposition of N2O5 overall?
Equilibrium can be disturbed, however, by the addition or removal of either a reactant or product. The graph on the right shows how the concentrations of the reactants and product of a reaction change when equilibrium is disturbed. Write the equation for the reaction depicted in the graph. Write the equilibrium constant expression for the reaction. Explain the shapes of the curves for the three gases during the first 2 minutes of the 4.
At approximately what time does the reaction reach equilibrium? How do you know equilibrium has been reached? What are the concentrations of the three gases at equilibrium? Calculate the value of Keq for the reaction. Describe the change made in the system 4 minutes into the reaction. Tell how you know the change was made. At what time does the system return to equilibrium?
Chlorine gas is added to the water in some large commercial swimming pools to kill bacteria. However, in most home swimming pools, either solid calcium hypochlorite Ca OCl 2 or an aqueous solution of sodium hypochlorite NaOCl is used to treat the water. Both compounds dissociate in water to form the weak acid hypochlorous acid HOCl. Hypochlorous acid is a highly effective bactericide.
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Use the information above to answer the following questions about the acid-base reactions that take place in swimming pools. Write an equation that shows the reaction between hypochlorous acid and water. Identify the acid, base, conjugate acid, and conjugate base in this reaction. Name the acid, base, conjugate acid, and conjugate base in this reaction. What effect does the addition of hypochlorite ion have on the pH of swimming pool water?
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The effectiveness of hypochlorite ion as a bactericide depends on pH. How does high pH affect the equilibrium reaction described in question 2? What effect would high pH have on the bacteria? In the presence of sunlight, hypochlorite ion decomposes to form chloride ion and oxygen gas. Write an equation for this reaction and tell how it affects the safety of pool water. One such method involves the use of a sacrificial metal. A sacrificial metal is a metal that is more easily oxidized than the metal it is designed to protect.
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Galvanized iron, for example, consists of a piece of iron metal covered with a thin layer of zinc. When galvanized iron is exposed to oxygen, it is the zinc, rather than the iron, that is oxidized. Water heaters often contain a metal rod that is made by coating a heavy steel wire with magnesium or aluminum. In this case, the magnesium or aluminum is the sacrificial metal, protecting the iron casing of the heater from corrosion.
The diagram shows a portion of a water heater containing a sacrificial rod. Answer the following questions about the diagram. Steel wire Sacrificial metal Iron casing Water 1. In the absence of a sacrificial metal, oxygen dissolved in water may react with the iron 2. Write the two half-reactions for this example of corrosion. Suppose the sacrificial rod in the diagram above is coated with aluminum metal.
Write the balanced equation for the reaction of aluminum with oxygen dissolved in the water.
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Hint: The product formed is aluminum hydroxide Al OH 3. Suppose that some iron in the casing of the water heater is oxidized, as shown in the equation of question 2 above. Write two half-reactions that represent this situation. Which element is oxidized and which is reduced in this reaction? For cells in which ion concentrations are greater or less than 1M, as shown below, an adjustment must be made to calculate cell potential. That adjustment is expressed by the Nernst equation: [product ion]x 0. Write the two half-reactions and the overall cell reaction for the cell shown above.
Use Table in your textbook to determine the standard potential of this cell. Write the Nernst equation for the cell. Calculate the cell potential for the ion concentrations shown in the cell. The structural formulas below are ten ways of representing compounds having the molecular formula C6H CH3 CH2 e. CH3 CH f. CH2 CH3 c. In the spaces provided, write the correct name for each of the structural formulas, labeled a—j, above.
How many different compounds are represented by the structural formulas above?