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Given the following heats of combustion: C2H2(g) = -1300 kJ/mole, H2(g) = -286 kJ/mole, C2H6(g) = -1560 kJ/mole, Calculate the enthalpy change for the following reaction C2H2(g)…

Given the following heats of combustion: C2H2(g) = -1300 kJ/mole, H2(g) = -286 kJ/mole, C2H6(g) = -1560 kJ/mole, Calculate the enthalpy change for the following reaction C2H2(g)…
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Given the following heats of combustion: C2H2(g) = -1300 kJ/mole, H2(g) = -286 kJ/mole, C2H6(g) = -1560 kJ/mole, Calculate the enthalpy change for the following reaction

C2H2(g) + 2H2(g) → C2H6(g)

a. -312 kJ

b. -26 kJ

c. +312 kJ

d. -26 kJ

User Serge Pavlov
by
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1 Answer

6 votes

Answer is A.

  • First plug in the designated enthalphy values for each
  • Then solve for the equation as you would an algebra problem
User Sasi V
by
8.0k points
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