Question

At 25 ∘c the reaction from part a has a composition as shown in the table below. Substancepressure (atm)c2h2(g)4.65h2(g)3.95c2h6(g)3.25×10−2 what is the free energy change, δg, in kilojoules for the reaction under these conditions? Express your answer numerically in kilojoules

Answer 1

Answer:

the free energy change in the kilojoules is, $21.05$ $kJ/mol$

Explanation:

•  $2H_{2} +C_{2} H_{2} ---- > C_{2} H_{6}$

•  $kp=$ $[C_{2} H_{6} ]/ [H_{2} ]^{2}$ x $[C_{2} H_{2}$$]$

              $= 1.25$ x $10^{-2}$ $/ [4.75]^{2}$ x $4.35$

              $=2.04$ x $10^{-4}$

• the basic formula for change in free energy is guven as,

            Δ$G$$=RT($㏑$kp$$)$

                  $=-8.314$ x $298k$ x ㏑$2.04$ x $10^{-4}$

                  $= 210485J/mol$

                 $= 21.05kJ/mol$

∴the free energy change in the kilojoules is, $21.05$ $kJ/mol$