107 763
Assignments Done
100%
Successfully Done
In June 2024

# Answer to Question #141187 in Inorganic Chemistry for Christine

Question #141187
3. Given the following thermochemical equations,
C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l) ∆H = -1299.5 KJ
C(s) + O2(g) → CO2(g) ∆H = -393.5 KJ
H2(g) + ½ O2(g) → H2O(l) ∆H = -285.8 KJ
Calculate ∆H for the decomposition of one mole of acetylene, C2H2(g), to its elements in their stable state at 25oC and 1 atm.
1
2020-10-30T06:43:26-0400

From the equations given;

"\\Delta_{H_a}=\\Delta_{H_b}+\\Delta_{H_c}"

The equation for the end reaction is;

"C_2H_2(-1299.5kJ)\\to 2CO_2(-393.5kJ)+H_2O(-285.8kJ)"

"\\Delta H\u00b0_D=\\Sigma \\Delta H\u00b0_{products}-\\Sigma \\Delta H\u00b0_{reactants}"

"=(-1299.5kJ)-[(2\\times -393.5kJ)+(-285.8kJ)]"

"=(-1299.5kJ)-(-1072.8kJ)"

"=-226.7kJ"

"\\Delta H\u00b0_D" For the reaction is therefore "-226.7kJ"

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!