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    Dalton'S Law of Partial Pressures

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    Liza Mae Neis
    The document discusses Dalton's law of partial pressures and gas stoichiometry. [1] Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gas components. [2] Gas stoichiometry uses the ideal gas law and balanced chemical equations to calculate amounts of gases involved in chemical reactions. [3] Sample problems demonstrate using these concepts to determine total pressure, moles of gas produced, and grams of gas produced.

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    Dalton'S Law of Partial Pressures

    Uploaded by

    Liza Mae Neis
    151 views3 pages
    The document discusses Dalton's law of partial pressures and gas stoichiometry. [1] Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gas components. [2] Gas stoichiometry uses the ideal gas law and balanced chemical equations to calculate amounts of gases involved in chemical reactions. [3] Sample problems demonstrate using these concepts to determine total pressure, moles of gas produced, and grams of gas produced.

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    Chemistry Report

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    The document discusses Dalton's law of partial pressures and gas stoichiometry. [1] Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gas components. [2] Gas stoichiometry uses the ideal gas law and balanced chemical equations to calculate amounts of gases involved in chemical reactions. [3] Sample problems demonstrate using these concepts to determine total pressure, moles of gas produced, and grams of gas produced.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
    151 views3 pages

    Dalton'S Law of Partial Pressures

    Uploaded by

    Liza Mae Neis
    The document discusses Dalton's law of partial pressures and gas stoichiometry. [1] Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gas components. [2] Gas stoichiometry uses the ideal gas law and balanced chemical equations to calculate amounts of gases involved in chemical reactions. [3] Sample problems demonstrate using these concepts to determine total pressure, moles of gas produced, and grams of gas produced.

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    © All Rights Reserved
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    DALTONS LAW OF PARTIAL PRESSURES

    -states that for a mixture of gases where no reaction takes place between the
    components, the total pressure is the sum of the partial pressures of the gas
    components

    Partial pressure: the pressure of each gas component; the pressure that the gas
    would exert alone [Note: Each gas behaves independently]

    Formula: = + + +..

    Sample Problem:

    1. A mixture contains carbon dioxide with a partial pressure of 125 mm Hg and


    oxygen with a partial pressure of 275 mm Hg. What is the total pressure of the
    mixture?

    Solution:

    = 2 + 2 = 125 + 275 = 400


    3. 4.30 moles of hydrogen gas is mixed with 2.20 moles of oxygen gas in a 10.0 L
    tank at 25.0 degrees Celsius. What is the total pressure inside the tank?

    = + = + = ; where = +

    MOLE FRACTION: The ratio of moles of one component of a gaseous mixture to


    the total number of moles of all components in the mixture. [Note: In any mixture,
    the sum of the mole fraction of all components is equal to 1.0]


    Formula: = = = and =

    Sample Problem:

    4. If a mixture of gases contains 7.50 g H2, 3.25 g O2, and 5.55 g N2. What is the
    mole fraction of each of the gases?
    GAS STOICHIOMETRY
    Stoichiometry: the study and calculation of quantitative relationships of the
    reactants and products in chemical reactions (chemical equations)

    Gas stoichiometry: involves chemical reactions that produces gases

    Key Points:

    At Standard Temperature and Pressure (STP), 1 mole of any gas will occupy a
    volume of 22.4 L.
    The Ideal Gas Law, along with a balanced chemical equation, can be used to
    solve for the amount, either in volume or mass, of gas consumed or
    produced in a chemical reaction.

    Sample Problem:

    1. () + () () + (

    According to the above reaction, what volume of 2 () is produced from the


    combustion of 100g of 3 (), assuming the reaction takes place at STP?

    2. () + () ()

    What volume of 3 will be formed from 12.0 L of 2 , if the volumes of the gases
    are measured under identical conditions of T and P? Assume that volume of 2
    supplied is an excess of that necessary to completely react all available 2 () and
    that the reaction goes by completion.

    3. () + () () + ()

    How many grams of 2 will be produced by 58.2 L of 4 at STP? Assume an


    excess of 2 ?

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