Regents Chemistry Test Preparation Practice

    Regents Test, Full Exam Practice Online: chemistry January 2012

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    Base your answers to questions 51 through 54 on the information below.

    The atomic radius and the ionic radius for some Group 1 and some Group 17 elements are given in the tables below.

    atom-and-the-ion fig: chem12012-exam_g13.png

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    Base your answers to questions 55 through 57 on the information below.

    Starting as a gas at 206°C, a sample of a substance is allowed to cool for 16 minutes. This process is represented by the cooling curve below.

    heating-curves-calculation-of-heat fig: chem12012-exam_g14.png

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    Base your answers to questions 58 and 59 on the information below.

    Two hydrocarbons that are isomers of each other are represented by the structural formulas and molecular formulas below.

    hydrocarbons fig: chem12012-exam_g15.png

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    Base your answers to questions 60 through 62 on the information below.

    The diagram below represents an operating electrolytic cell used to plate silver onto a nickel key. As the cell operates, oxidation occurs at the silver electrode and the mass of the silver electrode decreases.

    electrolytic-cell fig: chem12012-exam_g16.png

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    Base your answers to questions 63 through 65 on the information below.

    In a titration, a few drops of an indicator are added to a flask containing 35.0 milliliters of HNO3(aq) of unknown concentration. After 30.0 milliliters of 0.15 M NaOH(aq) solution is slowly added to the flask, the indicator changes color, showing the acid is neutralized.

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    Base your answers to questions 66 through 69 on the information below.

    During a fireworks display, salts are heated to very high temperatures. Ions in the salts absorb energy and become excited. Spectacular colors are produced as energy is emitted from the ions in the form of light.

    The color of the emitted light is characteristic of the metal ion in each salt. For example, the lithium ion in lithium carbonate, Li2CO3, produces a deep-red color. The strontium ion in strontium carbonate, SrCO3, produces a bright-red color. Similarly, calcium chloride is used for orange light, sodium chloride for yellow light, and barium chloride for green light.

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    Base your answers to questions 70 and 71 on the information below.

    A scientist makes a solution that contains 44.0 grams of hydrogen chloride gas, HCl(g), in 200. grams of water, H2O(ℓ), at 20.°C. This process is represented by the balanced equation below.

    solutions fig: chem12012-exam_g17.png

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    Base your answers to questions 72 through 74 on the information below.

    Iron has been used for thousands of years. In the air, iron corrodes. One reaction for the corrosion of iron is represented by the balanced equation below.

    Equation 1: 4Fe(s) + 3O2(g) → 2Fe2O3(s)

    In the presence of water, iron corrodes more quickly. This corrosion is represented by the unbalanced equation below.

    Equation 2: Fe(s) + O2(g) + H2O(ℓ) → Fe(OH)2(s)

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    Base your answers to questions 75 through 78 on the information below.

    Vitamin C, also known as ascorbic acid, is water soluble and cannot be produced by the human body. Each day, a person’s diet should include a source of vitamin C, such as orange juice. Ascorbic acid has a molecular formula of C6H8O6 and a gram-formula mass of 176 grams per mole.

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    Base your answers to questions 79 through 81 on the information below.

    Several steps are involved in the industrial production of sulfuric acid. One step involves the oxidation of sulfur dioxide gas to form sulfur trioxide gas. A catalyst is used to increase the rate of production of sulfur trioxide gas. In a rigid cylinder with a movable piston, this reaction reaches equilibrium, as represented by the equation below.

    2SO2(g) + O2(g) ⇌ 2SO3(g) + 392 kJ

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    Base your answers to questions 82 through 85 on the information below.

    Nuclear radiation is harmful to living cells, particularly to fast-growing cells, such as cancer cells and blood cells. An external beam of the radiation emitted from a radioisotope can be directed on a small area of a person to destroy cancer cells within the body.

    Cobalt-60 is an artificially produced radioisotope that emits gamma rays and beta particles. One hospital keeps a 100.0-gram sample of cobalt-60 in an appropriate, secure storage container for future cancer treatment.

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