Ask Question
3 May, 07:17

A 2.17 gm sample barium reacted completely with water what is the equation for the reaction how many milliliters of dry H2 evoled at 21degree celcius and 748mm of Hg?

+3
Answers (1)
  1. 3 May, 07:37
    0
    400 mL

    Explanation:

    Given dа ta:

    Mass of barium = 2.17 g

    Pressure = 748 mmHg (748/760 = 0.98 atm)

    Temperature = 21 °C (273 + 21 = 294k)

    Milliliters of H₂ evolved = ?

    Solution:

    chemical equation:

    Ba + 2H₂O → Ba (OH) ₂ + H₂

    Number of moles of barium:

    Number of moles = mass / molar mass

    Number of moles = 2.17 g / 137.327 g/mol

    Number of moles = 0.016 mol

    Now we will compare the moles of barium with H₂.

    Ba : H₂

    1 : 1

    0.016 : 0.016

    Milliliters of H₂:

    PV = nRT

    V = nRT/P

    V = 0.016 mol * 0.0821 atm. mol⁻¹. k⁻¹. L*294 k/0.98 atm

    V = 0.39 atm. L/0.98 atm

    V = 0.4 L

    L to mL

    0.4 * 1000 = 400 mL
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A 2.17 gm sample barium reacted completely with water what is the equation for the reaction how many milliliters of dry H2 evoled at ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers