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17 April, 01:03

A 0.200-g sample of cobalt metal reacted with hydrochloric acid according to the following balanced chemical equation: Co (s) + 2 HCl (aq) ➝ CoCl2 (aq) + H2 (g) The volume of hydrogen gas collected over water was 87.5 mL at 20 °C and a barometer reading of 763 mm Hg. Referring to Example Exercise 1, the adjusted volume of the H2 gas is

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  1. 17 April, 03:28
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    V H2 (g) = 83.13 mL

    Explanation:

    Dalton's law:

    Pgas = Pbar - P*H2O

    ∴ vapor pressure (P*)

    ⇒ P*H2O (20°C) = 17.5 mmHg

    ∴ Pbar = 763 mmHg

    ⇒ PH2 = 763 mmHg - 17.5 mmHg = 745.5 mmHg = 0.9809 atm

    Co (s) + 2 HCl (aq) → CoCl2 (aq) + H2 (g)

    ∴ Mw Co (s) = 58.933 g/mol

    ⇒ mol Co (s) = (0.200 g Co) * (mol/58.933 g) = 3.394 E-3 mol Co

    ⇒ n H2 (g) = (3.394 E-3 mol Co) (mol H2 / mol Co) = 3.394 E-3 mol H2 (g)

    ideal gas:

    PV = RTn

    ∴ R = 0.082 atm. L/K. mol

    ∴ T = 20°C ≅ 293 K

    the adjusted volume H2 (g):

    ⇒ V H2 (g) = ((0.082 atm. L/K. mol) (293 K) (3.394 E-3 mol)) / (0.9809 atm)

    ⇒ V H2 (g) = 0.08313 L

    ⇒ V H2 (g) = 83.13 mL
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