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4 October, 01:32

A laboratory assistant needs to prepare 35.2 liters of hydrogen at 25.0°C and 101.3 kilopascals. This is the equation for the reaction: 2HCl + Ca → H2 + CaCl2 What volume of 2.3 M hydrochloric acid is required to produce this much gas? Use the ideal gas resource. A. 0.625 L B. 0.876 L C. 1.18 L D. 1.25 L

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  1. 4 October, 01:55
    0
    Volume of hydrogen gas = 35.2L

    Temperature of hydrogen gas = 25.0°C + 273 = 298 K

    Pressure of hydrogen gas = 101.3 kPa = 1 atm

    (Conversion factor 1 atm = 101.325 kPa)

    Using the Ideal gas law,

    PV = nRT

    where P, V, n, R and T are pressure, volume, number of moles, universal gas constant and temperature respectively.

    n = PV/RT

    The number of moles of hydrogen gas,

    n = 35.2 L x 1 atm / 0.0821 L. atm. mol⁻¹1. K⁻¹ x 298 K

    n = 1.438 moles

    2HCl + Ca → H₂ + CaCl₂

    Based on the given balanced equation, 1 mole of H₂ is produced from two moles of HCl.

    Since H₂ is 1.438 moles, HCl will be (1.438 x 2) moles or 2.876 moles

    Given, Molarity of HCl = 2.3 M

    Molarity = moles of solute / liter of the solution

    Thus the volume of HCl is,

    2.3 M = 2.876 moles / liter of the solution

    V = 2.876 moles / 2.3 M

    V = 1.25 L

    Thus the volume of 2.3 M hydrochloric acid required to produce the given amount gas is 1.25 L.
  2. 4 October, 05:16
    0
    The answer is D. 1.25

    Explanation:

    Plato
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