InterviewSolution
Saved Bookmarks
InterviewSolution
| 1. |
When `12.0g` of `C` reacted with oxygen to form `CO` and `CO_(2)` at `25^(@)C` at constant pressure, `313.8 kJ` of heat was released and no carbon remained. Calculate the mass of oxygen which reacted. `Delta_(f)H^(Theta) (CO,g) =- 110.5 kJ mol^(-1)` and `Delta_(r)H^(Theta) (CO,g) =- 393.5 kJ mol^(-1)` |
|
Answer» `{:(C + (1)/(2)O_(2) rarr CO ,,DeltaH =- 110.5),(C+O_(2)rarrCO_(2),,DeltaH =- 393.5):}` Let `x mol` of `C` is converted into `CO` and `(1-x)` mol into `CO_(2)`. `:.x (-110.5) +(1-x)(-393.5) =- 313.8` `x = 0.2816 mol` Amount of `O_(2)` needed `= (0.2816)/(2) +(1-0.2816)` `= 0.8592 mol = 0.8592 xx 32` `= 27.5 g` |
|