50 g of iron reacts completely with two molar equivalents of hydrochloric acid i

Question

50 g of iron reacts completely with two molar equivalents of hydrochloric acid in solution, evolving gaseous H2 and generating the salt FeCl2. Calculate the pressure-volume work done by the evolved H2 gas under the following conditions. Use the ideal gas equation of state for all gases. a. In a closed vessel of fixed volume. b. In an open beaker at 25 °C, at 1 atm of pressure. If you are confused about what volume to use here, pretend the evolved H2 is collected in a massless, flimsy bag above the beaker.

Explanation / Answer

work done

Fe + 2HCl --> FeCl2 + H2

a. In a closed vessel of fixed volume

work done = 0 kJ

b. In an open vesel

moles of H2 produced = 50 g/55.845 g/mol

                                    = 0.895 mol

Volume (V) = nRT/P

                   = 0.895 x 0.08205 x 298

                   = 21.88 L

Work done = -1 x 21.88 x 101.33

                   = -2.217 kJ

Related Questions

Navigate

• Browse (All)
• Browse 5
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.