Question

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔH = -1.37x10^3 kJ What would happen to the value of ΔH for the reaction of ethanol with oxygen if each of the following occurred: If the reaction was reversed: 2CO2(g) + 3H2O(l) → C2H5OH(l) + 3O2(g) ΔH = 1.37x10^3 kJ If the reaction was multiplied by 2: 2C2H5OH(l) + 6O2(g) → 4CO2(g) + 6H2O(l) ΔH = -2.74x10^3 kJ If the water was (g) instead of (l): C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g) ΔH = -1.37x10^3 kJ If the ethanol was (g) instead of (l): C2H5OH(g) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔH = -1.37x10^3 kJ Is this reaction exothermic or endothermic: This reaction is exothermic.

          C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔH = -1.37x10^3 kJ

What would happen to the value of ΔH for the reaction of ethanol with oxygen if each of the following occurred:

If the reaction was reversed:
2CO2(g) + 3H2O(l) → C2H5OH(l) + 3O2(g) ΔH = 1.37x10^3 kJ

If the reaction was multiplied by 2:
2C2H5OH(l) + 6O2(g) → 4CO2(g) + 6H2O(l) ΔH = -2.74x10^3 kJ

If the water was (g) instead of (l):
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g) ΔH = -1.37x10^3 kJ

If the ethanol was (g) instead of (l):
C2H5OH(g) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔH = -1.37x10^3 kJ

Is this reaction exothermic or endothermic:
This reaction is exothermic.

Added by Celia S.

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