Question

2 co (g) + C (g) -> C3O2 (g)

delta h = 127.3 kJ/mol (rxn)
the equation above represents an endothermic reaction between CO(g) and C(g). What is the amount of heat absorbed when 1.00 mol of Co reacts with an excess C?

a) 31.8 kJ
b)63.7 kJ
c)127.3 kJ
d)254.6 kJ

Answer 1

b) 63.7 kJ

Step-by-step explanation:

`2 CO_((g))  + C _((s)) ----> C_(3)O_(2)`

we have ΔH = 127.3 kJ/mol

for 1.00 mole of CO the equation can be re-written as,

`CO_((g))  +(1)/(2)  C _((s)) ---->(1)/(2)  C_(3)O_(2)`

since the number of moles are halved ΔH also gets halved as per Hesse's law of constant summation,

ΔH =
`(127.3)/(2)`

= 63.7 kJ