What amount of carbon dioxide is produced per kJ of heat produced in burning ethene, C2H4?
The burning of a hydrocarbon will yield carbon dioxide and water.
C₂H₄ + 3 O₂ --> 2 CO₂ + 2 H₂O
From the balanced equation, 1 mol of C₂H₄ will produce 2 mol of CO₂. I'm not sure what to do besides looking up ΔH for the reaction.
Either look up the heat combustion of ethene or go to the delta Hformation stables and look up CO2, H2O, and ethene. Then dHrxn = (n*dHformation products) - (n*dHformation reactants)
To determine the amount of carbon dioxide (CO2) produced per kilojoule (kJ) of heat produced in burning ethene (C2H4), we need to use the balanced chemical equation for the combustion of ethene.
The balanced chemical equation for the combustion of ethene is:
C2H4 + 3 O2 → 2 CO2 + 2 H2O
From this equation, we can see that for every 1 mole of ethene (C2H4) burned, 2 moles of carbon dioxide (CO2) are produced.
To find the amount of CO2 produced per kJ of heat produced, we need to calculate the heat released during the combustion of ethene. The heat released can be determined by the enthalpy change of the reaction.
The enthalpy change for the combustion of ethene can be found in a thermodynamics reference book or online database. Let's assume that the enthalpy change is -1411.2 kJ/mol.
So, for every mole of ethene burned, the heat released is -1411.2 kJ.
Now, we can calculate the amount of CO2 produced per kJ of heat:
(2 moles CO2 / 1 mole C2H4) / (-1411.2 kJ / 1 mole C2H4) = -2 / 1411.2 ≈ -0.0014 moles CO2 per kJ of heat
Note that the negative sign in the calculations indicates that the reaction releases heat (exothermic).
Therefore, approximately 0.0014 moles of carbon dioxide (CO2) are produced per kJ of heat produced in the combustion of ethene, C2H4.