Regents Chemistry Test Preparation Practice

    Regents Test, Full Exam Practice Online: chemistry January 2016

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    Base your answers to questions 54 through 56 on the information below and on your knowledge of chemistry.

    The bright-line spectra observed in a spectroscope for three elements and a mixture of two of these elements are represented in the diagram below.

    excited-states-bright-line-spectrum fig: chem12016-exam_g6.png

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    Base your answers to questions 57 through 61 on the information below and on your knowledge of chemistry.

    The Lewis electron-dot diagrams for three substances are shown below.

    electron-dot-diagrams-(lewis-structures) fig: chem12016-exam_g7.png

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    Base your answers to questions 62 through 65 on the information below and on your knowledge of chemistry.

    A NaOH(aq) solution and an acid-base indicator are used to determine the molarity of an HCl(aq) solution. A 25.0-milliliter sample of the HCl(aq) is exactly neutralized by 15.0 milliliters of 0.20 M NaOH(aq).

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    Base your answers to questions 66 through 68 on the information below and on your knowledge of chemistry.

    Elements with an atomic number greater than 92 can be artificially produced in nuclear reactions by bombarding a naturally occurring nuclide with a different nuclide. One of these elements is roentgenium, Rg. The equation below represents a nuclear reaction that produces Rg-272.

    nucleus fig: chem12016-exam_g8.png

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    Base your answers to questions 69 through 72 on the information below and on your knowledge of chemistry.

    Hydrazine, N2H4, is a compound that is very soluble in water and has a boiling point of 113°C at standard pressure. Unlike water, hydrazine is very reactive and is sometimes used as a fuel for small rockets. One hydrazine reaction producing gaseous products is represented by the balanced equation below.

    N2H4(ℓ) → N2(g) + 2H2(g) + heat

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    Base your answers to questions 73 through 75 on the information below and on your knowledge of chemistry.

    A laboratory technician is given the table below and a sample of one of the three substances listed in the table. The technician makes an aqueous solution with a portion of the sample. When a conductivity tester is lowered into the solution, the lightbulb on the tester glows brightly. Another portion of the sample is placed in a heat-resistant container that is placed in an oven at 450.°C. The sample melts.

    differentiation-of-types-of-substances fig: chem12016-exam_g9.png

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    Base your answers to questions 76 through 78 on the information below and on your knowledge of chemistry.

    Natural gas and coal are two fuels burned to produce energy. Natural gas consists of approximately 80% methane, 10% ethane, 4% propane, 2% butane, and other components.

    The burning of coal usually produces sulfur dioxide, SO2(g), and sulfur trioxide, SO3(g), which are major air pollutants. Both SO2(g) and SO3(g) react with water in the air to form acids.

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    Base your answers to questions 79 through 82 on the information below and on your knowledge of chemistry.

    A student prepares two 141-gram mixtures, A and B. Each mixture consists of NH4Cl, sand, and H2O at 15°C. Both mixtures are thoroughly stirred and allowed to stand. The mass of each component used to make the mixtures is listed in the data table below.

    classification-of-matter fig: chem12016-exam_g10.png

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    Base your answers to questions 83 through 85 on the information below and on your knowledge of chemistry.

    Fossil fuels produce air pollution and may eventually be depleted. Scientists are researching ways to use hydrogen as an alternate fuel.

    A device called an artificial leaf was invented to produce hydrogen and oxygen using sunlight and water. The artifical leaf is an electrochemical cell. Equations 1 and 2 below represent the reactions taking place in the leaf. Equation 3 represents a reaction of hydrogen when used as fuel.

    Equation 1: 2H2O + energy from sunlight → O2 + 4H+ + 4e

    Equation 2: 4H+ + 4e → 2H2

    Equation 3: 2H2(g) + O2(g) → 2H2O(g) + energy

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