The free energy change for the following reactions are given below. C2H2(g)+(5/2)O2(g) xrightarrow[]2CO2(g)+H2O(l); Δ G° =-1234 kJ C(s)+O2(g) xrightarrowCO2(g); Δ G° =- 394 kJ H2(g)+(1/2)O2(g) xrightarrowH2O(l); Δ G° =- 237 kJ What is the standard free energy change for the reaction? H2(g)+2C(s) xrightarrowC2H2(g)

Question

The free energy change for the following reactions are given below. C2H2(g)+(5/2)O2(g) xrightarrow[]2CO2(g)+H2O(l); Δ G° =-1234 kJ C(s)+O2(g) xrightarrowCO2(g); Δ G° =- 394 kJ H2(g)+(1/2)O2(g) xrightarrowH2O(l); Δ G° =- 237 kJ What is the standard free energy change for the reaction? H2(g)+2C(s) xrightarrowC2H2(g)  (A)  - 209 text kJ  (B)  - 2259 text kJ  (C)  + 2259 text kJ  (D)  209 text kJ

Tardigrade Admin · Accepted Answer

C2H2(g)+(5/2)O2(g) xrightarrow2CO2(g)+H2O (l); Δ G° =-1234 kJ ?(i) C(s)+O2(g) xrightarrowCO2(g); Δ G° =- 394 kJ ?(ii) H2(g)+(1/2)O2(g) xrightarrowH2O(l); Δ G° =- 237 kJ ?(iii) Eq. 2(ii) + (iii) - (i) 2C(s)+H2(g) xrightarrowC2H2(g) Δ G° =2(-394)+(-237)-(-1234) Δ G° =209 kJ

$- 209 k J$

$- 2259 k J$

$+ 2259 k J$

$209 k J$

−209kJ

−2259kJ

+2259kJ

209kJ

C2​H2​(g)+25​O2​(g)​2CO2​(g)+H2​O(l); ΔG∘=−1234kJ ?(i) C(s)+O2​(g)​CO2​(g); ΔG∘=−394kJ ?(ii) H2​(g)+21​O2​(g)​H2​O(l); ΔG∘=−237kJ ?(iii) Eq. 2(ii) + (iii) - (i) 2C(s)+H2​(g)​C2​H2​(g) ΔG∘=2(−394)+(−237)−(−1234) ΔG∘=209kJ

$- 209 k J$

$- 2259 k J$

$+ 2259 k J$

$209 k J$