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?

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