Question

Using the reaction below: 2 CO2(g) + 2 H2O(l) → C2H4(g) + 3 O2(g) ΔHrxn= +1411.1 kJ What would be the heat of reaction for this reaction? 0.5 C2H4(g) + 1.5 O2(g) → CO2(g) + H2O(l) ΔHrxn= ??? KJ Question 6 options: a) Not enough information is given b) -2822.2 kJ c) +1411.1 kJ d) -705.55 kJ e) -1411.1 kJ

Answer 1

Answer: d) -705.55 kJ

Step-by-step explanation:

Heat of reaction is the change of enthalpy during a chemical reaction with all substances in their standard states.

`2CO_2(g)+2H_2O(l)\rightarrow C_2H_4(g)+3O_2(g)`
`\Delta H=+1411.1kJ`

Reversing the reaction, changes the sign of
`\Delta H`

`C_2H_4(g)+3O_2(g)\rightarrow 2CO_2(g)+2H_2O(l)`

`\Delta H=-1411.1kJ`

On multiplying the reaction by
`(1)/(2)` , enthalpy gets half:

`0.5C_2H_4(g)+1.5O_2(g)\rightarrow CO_2(g)+H_2O(l)`
`\Delta H=(1)/(2)* -1411.1kJ=-705.55kJ/mol`

Thus the enthalpy change for the given reaction is -705.55kJ