Syvum Home Page

Home > Examinations > NYSED Regents Exams > Chemistry > Print Preview

Physical Setting / Chemistry - New York Regents June 2012 Exam

Formats Worksheet / Test Paper Quiz Review

Hide all answers   View all answers   Print   Try the Quiz

Part A
Answer all questions in this part.
   Directions (1–30): For each statement or question, record on your separate answer sheet the number of the
word or expression that, of those given, best completes the statement or answers the question. Some questions
may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

1.
1 The mass of a proton is approximately equal to
  the mass of
  (1) an alpha particle   (3) a positron
  (2) a beta particle     (4) a neutron
Answer: 4

2.
2 An orbital of an atom is defined as the most
  probable location of
  (1) an electron        (3) a positron
  (2) a neutron          (4) a proton
Answer: 1

3.
3 What must occur when an electron in an atom
  returns from a higher energy state to a lower
  energy state?
  (1) A specific amount of energy is released.
  (2) A random amount of energy is released.
  (3) The atom undergoes transmutation.
  (4) The atom spontaneously decays.
Answer: 1


4.
4 Which element is a liquid at 305 K and
  1.0 atmosphere?
  (1) magnesium       (3) gallium
  (2) fluorine        (4) iodine
Answer: 3

5.
5 Which list of elements consists of a metal, a
  metalloid, and a nonmetal?
  (1) Li, Na, Rb          (3) Sn, Si, C
  (2) Cr, Mo, W           (4) O, S, Te
Answer: 3

6.
6 At STP, which physical property of aluminum
  always remains the same from sample to sample?
  (1) mass                 (3) length
  (2) density              (4) volume
Answer: 2

7.
7 Which statement describes a chemical property
  of silicon?
  (1) Silicon has a blue-gray color.
  (2) Silicon is a brittle solid at 20.°C.
  (3) Silicon melts at 1414°C.
  (4) Silicon reacts with fluorine.
Answer: 4

8.
8 Which diagram represents a mixture of two
  different molecular forms of the same element?

Answer: 1

9.
9 A compound is broken down by chemical means
  during
  (1) chromatography     (3) electrolysis
  (2) distillation       (4) filtration
Answer: 3

10.
10 Which quantities must be conserved in all
   chemical reactions?
   (1) mass, charge, density
   (2) mass, charge, energy
   (3) charge, volume, density
   (4) charge, volume, energy
Answer: 2

11.
11 Which phrase describes the distribution of
   charge and the polarity of a CH4 molecule?
   (1) symmetrical and polar
   (2) symmetrical and nonpolar
   (3) asymmetrical and polar
   (4) asymmetrical and nonpolar
Answer: 2

12.
12 What is the charge of the nucleus of an oxygen
   atom?
   (1) 0                    (3) +8
   (2) -2                   (4) +16
Answer: 3

13.
13 Which ion has no electrons?
   (1) H+                  (3) Na+
   (2) Li+                 (4) Rb+
Answer: 1

14.
14 To break a chemical bond, energy must be
   (1) absorbed           (3) produced
   (2) destroyed          (4) released
Answer: 1

15.
15 Which Lewis electron-dot diagram represents a
   nitrogen atom in the ground state?

Answer: 3

16.
16 What is the most likely electronegativity value
   for a metallic element?
   (1) 1.3                 (3) 3.4
   (2) 2.7                 (4) 4.0
Answer: 1

17.
17 Which polyatomic ion has a charge of 3-?
   (1) chromate ion       (3) phosphate ion
   (2) oxalate ion        (4) thiocyanate ion
Answer: 3

18.
18 Every chlorine atom has
   (1) 7 electrons
   (2) 17 neutrons
   (3) a mass number of 35
   (4) an atomic number of 17
Answer: 4

19.
19 Which substance can not be broken down by a
   chemical change?
   (1) ammonia            (3) propane
   (2) methanol           (4) phosphorus
Answer: 4

20.
20 At standard pressure, which substance becomes
   less soluble in water as temperature increases
   from 10.°C to 80.°C?
   (1) HCl                  (3) NaCl
   (2) KCl                  (4) NH4Cl
Answer: 1

21.
21 Which type of concentration is calculated when
   the grams of solute is divided by the grams of
   the solution, and the result is multiplied by
   1 000 000?
   (1) molarity             (3) percent by mass
   (2) parts per million    (4) percent by volume
Answer: 2

22.
22 Which type of energy is associated with the
   random motion of atoms and molecules in a
   sample of air?
   (1) chemical energy   (3) nuclear energy
   (2) electrical energy (4) thermal energy
Answer: 4

23.
23 The temperature of a sample of matter is a
   measure of the
   (1) total kinetic energy of the particles in the
       sample
   (2) total potential energy of the particles in the
       sample
   (3) average potential energy of the particles in
       the sample
   (4) average kinetic energy of the particles in the
       sample
Answer: 4

24.
24 Which unit is used to express the pressure of a
   gas?
   (1) mole                (3) kelvin
   (2) joule               (4) pascal
Answer: 4

25.
25 Which sample of matter sublimes at room
   temperature and standard pressure?
   (1) Br2(ℓ)             (3) CO2(s)
   (2) Cl2(g)             (4) SO2(aq)
Answer: 3

26.
26 Given the diagram representing a closed system
   at constant temperature:
Which statement describes this system at
equilibrium?
(1) The mass of H2O(ℓ) equals the mass of
    H2O(g).
(2) The volume of H2O(ℓ) equals the volume of
    H2O(g).
(3) The number of moles of H2O(ℓ) equals the
    number of moles of H2O(g).
(4) The rate of evaporation of H2O(ℓ) equals
    the rate of condensation of H2O(g).
Answer: 4

27.
27 Which reaction occurs at the cathode in an
   electrochemical cell?
   (1) combustion        (3) oxidation
   (2) neutralization    (4) reduction
Answer: 4

28.
28 Which substance yields H+(aq) as the only
   positive ion in an aqueous solution?
   (1) CH3CHO               (3) CH3COOH
   (2) CH3CH2OH             (4) CH3OCH3
Answer: 3

29.
29 Compared to the mass and the penetrating
   power of an alpha particle, a beta particle has
   (1) less mass and greater penetrating power
   (2) less mass and less penetrating power
   (3) more mass and greater penetrating power
   (4) more mass and less penetrating power
Answer: 1

30.
30 During a nuclear reaction, mass is converted
   into
   (1) charge             (3) isomers
   (2) energy             (4) volume
Answer: 2


Part B–1
Answer all questions in this part.
   Directions (31–50): For each statement or question, record on your separate answer sheet the number of the
word or expression that, of those given, best completes the statement or answers the question. Some questions
may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

31.
31 An atom in the ground state has two electrons in
   its first shell and six electrons in its second shell.
   What is the total number of protons in the
   nucleus of this atom?
   (1) 5                         (3) 7
   (2) 2                         (4) 8
Answer: 4

32.
32 A bromine atom in an excited state could have
   an electron configuration of
   (1) 2-8-18-6             (3) 2-8-17-7
   (2) 2-8-18-7             (4) 2-8-17-8
Answer: 4

33.
33 The atomic masses and the natural abundances
   of the two naturally occurring isotopes of
   lithium are shown in the table below.
                Lithium Isotopes
                                  
     Isotope     Atomic Mass     Natural Abundance
                         (u)                    (%)
       Li-6          6.02             7.5
       Li-7          7.02            92.5
   Which numerical setup can be used to deter-
   mine the atomic mass of lithium?
   (1) (0.075)(6.02 u) + (0.925)(7.02 u)
   (2) (0.925)(6.02 u) + (0.075)(7.02 u)
   (3) (7.5)(6.02 u) + (92.5)(7.02 u)
   (4) (92.5)(6.02 u) + (7.5)(7.02 u)
Answer: 1

34.
34 Element X reacts with chlorine to form an ionic
   compound that has the formula XCl2. To which
   group on the Periodic Table could element X
   belong?
   (1) Group 1             (3) Group 13
   (2) Group 2             (4) Group 15
Answer: 2

35.
35 Which general trend is found in Period 3 as the
   elements are considered in order of increasing
   atomic number?
   (1) increasing atomic radius
   (2) increasing electronegativity
   (3) decreasing atomic mass
   (4) decreasing first ionization energy
Answer: 2

36.
36 Given the formula for a compound:
Which molecular formula and empirical formula
represent this compound?
(1) C2HNO2 and CHNO
(2) C2HNO2 and C2HNO2
(3) C4H2N2O4 and CHNO
(4) C4H2N2O4 and C2HNO2
Answer: 4

37.
37 What is the gram-formula mass of (NH4)3PO4?
   (1) 112 g/mol          (3) 149 g/mol
   (2) 121 g/mol          (4) 242 g/mol
Answer: 3

38.
38 In the ground state, which atom has a completely
   filled valence electron shell?
   (1) C                      (3) Ne
   (2) V                      (4) Sb
Answer: 3

39.
39 Given the formula:
The bond between which two atoms has the
greatest degree of polarity?
(1) C and C               (3) H and C
(2) C and O               (4) H and O
Answer: 4

40.
40 Given the diagram representing a heating curve
   for a substance:
                    Heating Curve
During which time interval is the average kinetic
energy of the particles of the substance constant
while the potential energy of the particles
increases?
(1) AC                     (3) CD
(2) BC                     (4) DF
Answer: 2

41.
41 At 50.°C and standard pressure, intermolecular
   forces of attraction are strongest in a sample of
   (1) ethanoic acid          (3) propanone
   (2) ethanol                (4) water
Answer: 1

42.
42 At 101.3 kPa and 298 K, what is the total
   amount of heat released when one mole of
   aluminum oxide, Al2O3(s), is formed from its
   elements?
   (1) 393.5 kJ          (3) 1676 kJ
   (2) 837.8 kJ          (4) 3351 kJ
Answer: 3

43.
43 Given the balanced equation representing a
   reaction:
       2H2O(ℓ) + 571.6 kJ → 2H2(g) + O2(g)
   What occurred as a result of this reaction?
   (1) Energy was absorbed, and entropy increased.
   (2) Energy was absorbed, and entropy decreased.
   (3) Energy was released, and entropy increased.
   (4) Energy was released, and entropy decreased.
Answer: 1

44.
44 Given the potential energy diagram representing
   a reversible reaction:
The activation energy for the reverse reaction is
represented by
(1) A + B                (3) B + D
(2) B + C                (4) C + D
Answer: 2

45.
45 Which formula represents a molecule of
   2-chlorobutane?

Answer: 2

46.
46 Which formula represents an unsaturated
   hydrocarbon?
   (1) CH4             (3) C3H8
   (2) C2H4            (4) C4H10
Answer: 2

47.
47 Which ion is most easily reduced?
   (1) Zn2+                 (3) Co2+
   (2) Mg2+                 (4) Ca2+
Answer: 3

48.
48 Given the balanced equation representing a
   reaction:
  HSO4-(aq) + H2O(ℓ) → H3O+(aq) + SO42-(aq)
   According to one acid-base theory, the H2O(ℓ )
   molecules act as
   (1) a base because they accept H+ ions
   (2) a base because they donate H+ ions
   (3) an acid because they accept H+ ions
   (4) an acid because they donate H+ ions
Answer: 1

49.
49 Which equation represents an oxidation-
   reduction reaction?
   (1) H+ + OH- → H2O
(3) Zn + Sn4+ → Zn2+ + Sn2+
(4) 3AgNO3 + Li3PO4 → Ag3PO4 + 3LiNO3
Answer: 3

50.
50 Which equation represents natural transmutation?
(3) S + 2e- → S2-
(4) Na → Na+ + e-
Answer: 2


Part B–2
Answer all questions in this part.
   Directions (51–65): Record your answers in the spaces provided in your answer booklet. Some questions
may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

51.
51 What is the mass of KNO3(s) that must dissolve in 100. grams of water to form a
   saturated solution at 50.°C? [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for 84 g ± 2 g.


52.
Base your answers to questions 52 through 55 on the information below.
         The reaction between aluminum and an aqueous solution of copper(II) sulfate is
      represented by the unbalanced equation below.
                            Al(s) + CuSO4(aq) → Al2(SO4)3(aq) + Cu(s)
      52 Identify the type of chemical reaction represented by the equation. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             single replacement
             redox


53.
53 Balance the equation in your answer booklet, using the smallest whole-number
   coefficients. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for 
  2  Al(s) +  3  CuSO4(aq) → _______ Al2(SO4)3(aq) +  3  Cu(s).
        Allow credit even if the coefficient “1” is written in front of Al2(SO4)3(aq).


54.
54 Explain why the equation represents a chemical change. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             The products are different substances with different properties from the reactants.
             There is a loss and gain of electrons by substances in the reaction.


55.
55 Determine the total mass of Cu produced when 1.08 grams of Al reacts completely with
   9.58 grams of CuSO4 to produce 6.85 grams of Al2(SO4)3. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for 3.81 g.


56.
Base your answers to questions 56 through 59 on the information below.
          A total of 1.4 moles of sodium nitrate is dissolved in enough water to make 2.0 liters of
      an aqueous solution. The gram-formula mass of sodium nitrate is 85 grams per mole.
      56 Write the chemical formula for the solute in the solution. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for NaNO3.


57.
57 Show a numerical setup for calculating the mass of the solute used to make the solution. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             (85 g/mol)(1.4 mol)
             (1.4)(85)


58.
58 Compare the boiling point of the solution at standard pressure to the boiling point of
   H2O at standard pressure. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             At standard pressure, the boiling point of the solution is higher than the boiling point of H2O.
             Water boils at a lower temperature.


59.
59 Determine the molarity of the solution. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for 0.70 M. Significant figures do not need to be shown.


60.
Base your answers to questions 60 through 62 on the information below.
          Calcium reacts with water. This reaction is represented by the balanced equation below.
      The aqueous product of this reaction can be heated to evaporate the water, leaving a white
      solid, Ca(OH)2(s).
                              Ca(s) + 2H2O(ℓ) → Ca(OH)2(aq) + H2(g)
      60 Compare the electrical conductivity of the aqueous product in the reaction to the
         electrical conductivity of the white solid that remains after the water is evaporated from
         the solution. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             The solution can conduct an electric current better than the white solid.
             The Ca(OH)2(aq) is a good conductor and Ca(OH)2(s) is not.


61.
61 Write the chemical name of the base produced in the reaction. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for calcium hydroxide.


62.
62 State one change in reaction conditions that will increase the rate of the reaction. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             Increase the temperature of the water.
             Increase the surface area of Ca(s).


63.
Base your answers to questions 63 through 65 on the information below.
          In a titration, 20.0 milliliters of 0.15 M HCl(aq) is exactly neutralized by 18.0 milliliters
      of KOH(aq).
      63 Complete the equation in your answer booklet for the neutralization reaction by
         writing the formula of each product. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             H2O(ℓ) and KCl(aq)
             KCl and HOH


64.
64 Compare the number of moles of H+(aq) ions to the number of moles of OH-(aq) ions
   in the titration mixture when the HCl(aq) is exactly neutralized by the KOH(aq). [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             The number of moles of H+(aq) ions equals the number of moles of OH-(aq) ions.
             The number of hydrogen ions is the same as the number of hydroxide ions.


65.
65 Determine the concentration of the KOH(aq). [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for 0.17 M. Significant figures do not need to be shown.



Part C
Answer all questions in this part.
   Directions (66–85): Record your answers in the spaces provided in your answer booklet. Some questions
may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.

66.
Base your answers to questions 66 through 68 on the information below.
          John Dalton, an early scientist, sketched the structure of compounds using his own
      symbols for the elements known at the time. Dalton’s symbols for four elements and
      his drawing of potassium aluminum sulfate are represented by the diagram below.
                                      Dalton’s Drawing for
                                  Potassium Aluminum Sulfate
    Today, it is known that the chemical formula for potassium aluminum sulfate is
KAl(SO4)2 •12H2O. It is a hydrated compound because water molecules are included
within its crystal structure. There are 12 moles of H2O for every 1 mole of KAl(SO4)2.
The compound contains two different positive ions. The gram-formula mass of
KAl(SO4)2 •12H2O is 474 grams per mole.
66 Identify one positive ion in the hydrated compound. Your response must include both
   the chemical symbol and charge of the ion. [1]
Answer: MODEL ANSWER GIVEN BELOW
66 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
             K+
             Al3+


67.
67 Describe, in terms of composition, one way in which Dalton’s perception of potassium
   aluminum sulfate differs from what is known today about the compound. [1]
Answer: MODEL ANSWER GIVEN BELOW
67 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
             Dalton’s drawing did not include the element hydrogen.
             He perceived 5 sulfur atoms, but the formula actually has 2 sulfur atoms.
             Dalton’s drawing had more aluminum.
             It did not include water.


68.
68 Show a numerical setup for calculating the percent composition by mass of water in
   KAl(SO4)2•12H2O. [1]
Answer: MODEL ANSWER GIVEN BELOW
68 [1] Allow 1 credit. Acceptable responses include, but are not limited to:


69.
Base your answers to questions 69 through 71 on the information below.
          At standard pressure, hydrogen peroxide, H2O2, melts at -0.4°C, boils at 151°C, and is
      very soluble in water. A bottle of aqueous hydrogen peroxide, H2O2(aq), purchased from a
      pharmacy has a pressure-releasing cap. Aqueous hydrogen peroxide decomposes at room
      temperature, as represented by the balanced equation below.
                             2H2O2(aq) → 2H2O(ℓ) + O2(g) + 196.0 kJ
      69 State, in terms of both melting point and boiling point, why H2O2 is a liquid at room
         temperature. [1]
Answer: MODEL ANSWER GIVEN BELOW
69 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
             Room temperature is above the melting point and below the boiling point of H2O2.
             Room temperature is between -0.4°C and 151°C.
             -0.4°C < room temperature < 151°C


70.
70 State evidence that indicates the decomposition of H2O2(aq) is exothermic. [1]
Answer: MODEL ANSWER GIVEN BELOW
70 [1] Allow 1 credit. Acceptable responses include, but are not limited to:
             More energy is released than absorbed.
             Heat is a product of the reaction.


71.
71 Explain why a hydrogen peroxide bottle needs a pressure-releasing cap. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             The excess pressure due to the production of oxygen gas in the bottle needs to be gradually
             released.
             As O2 (g) is produced, the pressure inside of the bottle might increase and the bottle might burst
             without the pressure-releasing cap.


72.
Base your answers to questions 72 through 75 on the information below.
          A student constructs an electrochemical cell during a laboratory investigation. When
      the switch is closed, electrons flow through the external circuit. The diagram and equation
      below represent this cell and the reaction that occurs.
                        2Al(s) + 3Ni2+(aq) → 2Al3+(aq) + 3Ni(s)
72 State the direction of electron flow through the wire when the switch is closed. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             Electrons flow from the Al electrode to the Ni electrode.
             Electrons move left to right through the wire.


73.
73 Write a balanced half-reaction equation for the oxidation that occurs when the switch is
   closed. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             Al → 3e- + Al3+
             2Al → 2Al3+ + 6e-


74.
74 Determine the number of moles of Al(s) needed to completely react with 9.0 moles of
   Ni2+(aq) ions. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for 6.0 mol. Significant figures do not need to be shown.


75.
75 State, in terms of energy, why this cell is a voltaic cell. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             A spontaneous reaction converts chemical energy to electrical energy.
             A battery is not required to provide energy for the cell to operate.


76.
Base your answers to questions 76 through 78 on the information below.
          The diagram below shows typical pH values found in four parts of the human digestive
      system. In the small intestine, the enzyme lipase acts as a catalyst, increasing the rate of fat
      digestion.
76 Which labeled part of the digestive system has the most acidic environment? [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             stomach
             the organ with a pH of 2


77.
77 What is the color of thymol blue at the pH of the small intestine? [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for yellow.


78.
78 State how the catalyst lipase increases the rate of the fat digestion. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             The lipase provides an alternate reaction pathway that requires less energy.
             lower activation energy


79.
Base your answers to questions 79 through 81 on the information below.
          One type of soap is produced when ethyl stearate and sodium hydroxide react.
      The soap produced by this reaction is called sodium stearate. The other product of the
      reaction is ethanol. This reaction is represented by the balanced equation below.
 Ethyl stearate       Sodium hydroxide    Sodium stearate      Ethanol
79 Identify the type of organic reaction used to make soap. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for saponification.


80.
80 To which class of organic compounds does ethyl stearate belong? [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for ester or esters.


81.
81 Identify the two types of bonds in the compound sodium stearate. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             covalent bonds and ionic bonds
             polar and nonpolar
             single and double


82.
Base your answers to questions 82 through 85 on the information below.
          Nuclear fission has been used to produce electricity. However, nuclear fusion for
      electricity production is still under development. The notations of some nuclides used in
      nuclear reactions are shown in the table below.
                           Some Nuclides Used in Nuclear Reactions
82 Compare the atomic masses of nuclides used in fusion to the atomic masses of nuclides
   used in fission. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             The nuclides used for fusion have smaller atomic masses than nuclides used for fission.
             The nuclides used in fission are many times more massive.
             Fusion particles are lighter.


83.
83 Complete the table in your answer booklet that compares the total number of protons
   and the total number of neutrons for the hydrogen nuclides used for fusion. [1]
Answer: MODEL ANSWER GIVEN BELOW
83 [1] Allow 1 credit for the correct number of protons and the correct number of neutrons for both
       hydrogen nuclides.
        Example of a 1-credit response:


84.
84 Complete the nuclear equation in your answer booklet for the fission of   23592U   by
                                                                              
   writing the notation of the missing product. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit for 10n.
                            


85.
85 State one potential benefit of using nuclear fusion instead of the current use of nuclear
   fission to produce electricity. [1]
Answer: MODEL ANSWER GIVEN BELOW
 Allow 1 credit. Acceptable responses include, but are not limited to:
             Fusion produces more energy per gram of reactant.
             The fusion process produces less radioactive waste.
             The fusion reactant material is more readily available.



  Try the Quiz :     Physical Setting / Chemistry - New York Regents June 2012 Exam


Contact Info © 1999-2017 Syvum Technologies Inc. Privacy Policy Disclaimer and Copyright
Previous
-
Next
-