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    Ws 2 Stoichiometry

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    AlbertKoretzky
    This document contains a 20 question multiple choice chemistry worksheet covering topics in stoichiometry including: determining empirical formulas from percentage composition, calculating amounts of products from balanced reactions, identifying combustion reactions, and determining molecular formulas from molecular weight and percentage composition data. The questions require applying concepts like mole-mass conversions, using balanced chemical equations, and solving multiple step stoichiometry problems.

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    Ws 2 Stoichiometry

    Uploaded by

    AlbertKoretzky
    203 views2 pages
    This document contains a 20 question multiple choice chemistry worksheet covering topics in stoichiometry including: determining empirical formulas from percentage composition, calculating amounts of products from balanced reactions, identifying combustion reactions, and determining molecular formulas from molecular weight and percentage composition data. The questions require applying concepts like mole-mass conversions, using balanced chemical equations, and solving multiple step stoichiometry problems.

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    This document contains a 20 question multiple choice chemistry worksheet covering topics in stoichiometry including: determining empirical formulas from percentage composition, calculating amounts of products from balanced reactions, identifying combustion reactions, and determining molecular formulas from molecular weight and percentage composition data. The questions require applying concepts like mole-mass conversions, using balanced chemical equations, and solving multiple step stoichiometry problems.

    Copyright:

    © All Rights Reserved
    Download as RTF, PDF, TXT or read online from Scribd
    Download as rtf, pdf, or txt
    203 views2 pages

    Ws 2 Stoichiometry

    Uploaded by

    AlbertKoretzky
    This document contains a 20 question multiple choice chemistry worksheet covering topics in stoichiometry including: determining empirical formulas from percentage composition, calculating amounts of products from balanced reactions, identifying combustion reactions, and determining molecular formulas from molecular weight and percentage composition data. The questions require applying concepts like mole-mass conversions, using balanced chemical equations, and solving multiple step stoichiometry problems.

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    © All Rights Reserved
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    Download as rtf, pdf, or txt
    of 2

    GC Cal 2 Engr. Rugi Vicente C.

    Rubi (2nd Sem SY 14-15)


    Worksheet 1: Stoichiometry
    Name___________________________________
    MULTIPLE CHOICE. Choose the one alternative that best
    completes the statement or answers the question.
    1) What is the empirical formula of a compound that contains
    49.4% K, 20.3% S, and 30.3% O by mass?
    A) K2SO4
    B) KSO3 C) K2SO3
    D) KSO2

    E) KSO4

    2) If the reaction yield is 94.4%, what mass in grams of


    hydrogen is produced by the reaction of 4.73 g of magnesium
    with 1.83 g of water?
    Mg (s) + 2H2O (l) Mg(OH)2 (s) + H2 (g)
    A) 0.0485
    B) 0.219 C) 0.204
    D) 0.0162
    E) 0.0962
    3) Lead (II) carbonate decomposes to give lead (II) oxide and
    carbon dioxide:
    PbCO3 (s) PbO (s) + CO2 (g)

    11) How many atoms of nitrogen are in 10 g of NH4NO3?


    A) 3.0 1023
    B) 1.5 1023
    C) 2
    D) 1.8 E) 3.5
    12) When a hydrocarbon burns in air, what component of air
    reacts?
    A) water
    B) nitrogen
    C) carbon dioxide
    D) argon
    E) oxygen
    13) Which of the following are combustion reactions?
    1) CH4 (g) + O2 (g) CO2 (g) + H2O (l)
    2) CaO (s) + CO2 (g) CaCO3 (s)
    3) PbCO3 (s) PbO (s) + CO2 (g)

    4) CH3OH (l) + O2 (g) CO2 (g) + H2O (l)


    A) 2, 3, and 4
    B) 1, 3, and 4
    C) 3 and 4
    D) 1 and 4
    E) 1, 2, 3, and 4
    14) A nitrogen oxide is 63.65% by mass nitrogen. The molecular
    formula could be ________.
    A) NO2
    B) N2O
    C) NO

    D) N2O4
    E) either NO2 or N2O4
    How many grams of lead (II) oxide will be produced by the
    15) When the following equation is balanced, the coefficient of
    decomposition of 2.50 g of lead (II) carbonate?
    H2 is ________.
    A) 2.61 B) 0.00936
    C) 0.41 D) 2.50 E) 2.09
    K (s) + H2O (l) KOH (aq) + H2 (g)
    4) Calculate the percentage by mass of nitrogen in PtCl 2(NH3)2.
    A) 1
    B) 5
    C) 3
    D) 4
    E) 2
    A) 4.95 B) 4.67
    C) 9.90
    D) 9.34 E) 12.67
    16)
    The
    combustion
    of
    ammonia
    in
    the presence of excess
    5) The formula weight of potassium dichromate (K2Cr2O7) is
    oxygen yields NO2 and H2O:
    ________ amu.
    4 NH3 (g) + 7 O2 (g) 4 NO2 (g) + 6 H2O (g)
    A) 242.18
    B) 255.08
    C) 294.18
    The combustion of 43.9 g of ammonia produces ________ g of
    D) 107.09
    E) 333.08
    6) What mass in grams of hydrogen is produced by the reaction NO2.
    of 4.73 g of magnesium with 1.83 g of water?
    Mg (s) + 2H2O (l) Mg(OH)2 (s) + H2 (g)

    A) 178 B) 43.9 C) 2.58


    D) 0.954
    E) 119
    17) Which one of the following substances is the product of this
    combination reaction?
    Al (s) + I2(s) ________

    A) 0.0485
    B) 0.219
    C) 0.102
    D) 0.204
    E) 0.0162
    7) When the following equation is balanced, the coefficients are A) Al3I2 B) AlI3 C) Al2I3 D) AlI2 E) AlI
    ________.
    18) A compound is composed of only C, H, and O. The
    C8H18 + O2 CO2 + H2O
    combustion of a 0.519-g sample of the compound yields 1.24 g
    A) 4, 4, 32, 36
    B) 2, 25, 16, 18 C) 1, 4, 8, 9
    of CO2 and 0.255 g of H2O. What is the empirical formula of the
    D) 2, 3, 4, 4
    E) 2, 12, 8, 9
    compound?
    8) What is the maximum mass in grams of NH3 that can be
    A) C6H6O
    B) C2H6O5
    C) C3H3O
    produced by the reaction of
    of N2 with
    of H2 via the D) C2H6O2
    E) CH3O

    equation below?
    19) The combustion of propane (C3H8) produces CO2 and H2O:
    N2 (g) + H2 (g) NH3 (g) (not balanced)
    C3H8 (g) + 5O2 (g) 3CO2 (g) + 4H2O (g)
    A) 17 B) 0.61 C) 2.0 D) 1.2 E) 4.0
    The reaction of 2.5 mol of O2 with 4.6 mol of C3H8 will produce
    9) How many molecules of CH4 are in 48.2 g of this compound?
    ________ mol of H2O.
    A) 1.81 1024 B) 5.00 1024
    C) 3.00 D) 4.00
    A) 4.0
    B) 3.0
    C) 2.5 D) 2.0
    E) 1.0
    E) 2.90 1025
    20) A compound contains 40.0% C, 6.71% H, and 53.29% O by
    10) Pentacarbonyliron (Fe(CO)5) reacts with phosphorous
    mass. The molecular weight of the compound is 60.05 amu. The
    molecular formula of this compound is ________.
    trifluoride (PF3) and hydrogen, releasing carbon monoxide:
    A) C2H2O4
    B) CH2O
    C) C2H3O4
    Fe(CO)5 + PF3 + H2 Fe(CO)2(PF3)2(H)2 + CO
    E) CHO2
    The reaction of 5.0 mol of Fe(CO)5, 8.0 mol of PF3 and 6.0 mol of D) C2H4O2
    H2 will release ________ mol of CO.
    A) 24 B) 5.0 C) 12 D) 15 E) 6.0

    1) C
    2) E
    3) E
    4) D
    5) C
    6) C
    7) B
    8) D
    9) A
    10) C

    11) B
    12) E
    13) D
    14) B
    15) A
    16) E
    17) B
    18) C
    19) D
    20) D

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