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The commercial production of water gas u...

The commercial production of water gas utilizes the reaction under standard conditions `:C+H_(2)O_((g)) rarr H_(2)+CO`. The heat required for this endothermic reaction may be supplied by adding a limited amount of air and burning some carbon to `CO_(20`. How many gram of carbon must be burnt to `CO_(2)` to provide enough heat for the water gas conversion of `100g` carbon ? Neglect all heat losses to the environment. Also `DeltaH_(f)^(@)` of `CO,H_(2)O_((g))` and `CO_(2)` are `-110.53, -241.81` and `-393.51kJ //mol` respectively.

A

30.5 g

B

39.7 g

C

33.36 g

D

42.5 g

Text Solution

Verified by Experts

The correct Answer is:
C
`C + H_(2)O (g) rarr H_(2)(g) + CO_(g) " "Delta H_(f)^(@) = ?`
`:. " " DeltaH^@ = Delta_(f) H_(CO)^(@) = -110.53 - (-241 . 81) = 131.28 kJ//mol ( :' Delta_(f)H^@` for C and `H_2` are zero)
Thus, `DeltaH^@ `needed for 100 g carbon = `(131.28 xx 100)/(12) kJ`
Now, 393.51 kJ energy is provided by 12 g C
`(131.28 xx 100)/(12) kJ " energy is provided by" =(12 xx 131.28 xx 100)/(12 xx 393.51) = 33.36 g`
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