Consider the reaction. 2c(s, graphite) h2= c2h2(g) based on the equation and the information in the table, what is the enthalpy of the reaction?
a.453.46 kj
b.-226.73 kj (not this one, i got it wrong)
c.226.73 kj
d.453.46 kj

Delta H reaction (ΔH) is the amount of heat change between the system and its environment

(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)

The change in enthalpy in the formation of 1 mole of the elements is called enthalpy of formation

Delta H reaction (ΔH) is the difference between product enthalpy and reactant enthalpy (Hp-Hr)

Reaction :

2C + H2 -> C2H2

(ΔH) reaction = (ΔH) product - (ΔH) reactants

(ΔH) reaction = (ΔH) C2H2 - ((ΔH) C + (ΔH) H2)

for free element (ΔH) it has zero value, so (ΔH) C and (ΔH) H2 have zero value

From the available data: Hf (kJ / mol) C2 H2 (g)=  226.73

then

(ΔH) reaction = ΔH) C2H2 - ((ΔH) C + (ΔH) H2)

(ΔH) reaction = 226.73 - (0 + 0)

(ΔH) reaction = 226.73 (answer C)

(ΔH) reaction

Keywords : (ΔH) reaction, C2H2

C. 226.73 kJ

Explanation:

this is correct on ed-genuity, hope this helps! :)

idk

explanation:

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