Question
Use the standard enthalpies of formation for the reactants and products to solve for the ΔHrxn for the following reaction. (The ΔHf of C2H4 is 52.26 kJ/mol, CO2 is -393.509 kJ/mol, and H2O is -241.818 kJ.)
C2H4 (g) + 3O2(g) 2CO2 (g) + 2H2O(g)
ΔHrxn =
The reaction is .
C2H4 (g) + 3O2(g) 2CO2 (g) + 2H2O(g)
ΔHrxn =
The reaction is .
Answers
Related Questions
The equation for the complete combustion of ethene (C2H4) is
C2H4(g) + 3 O2(g) ==> 2CO2(g) + 2H2O(g...
C2H4(g)+ 3O2(g) --> 2 CO2 (g) + 2H2O (l)
The complete combustion of 11.22g of ethylene, C2H4 (g), v...
Given the following data:
C2H4 (g) + 3O2 (g) -> 2CO2 (g) + 2H2O (l) H = –1411.0 kJ
2C2H6 (g) + 7O2...
Which of the following reactions is exothermic?
Question 4 options:
a) C2H4(g) + O2(g) → 2C(s) +...