I've got a really hard question here, hope someone can help me here!
1. 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) ∆H = -2600 kJ The energy released when 0.5 mole of each gas is mixed and ignited is A 260 kJ B 520 kJ C 650 kJ D 1300 kJ
I've got a really hard question here, hope someone can help me here!
1. 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) ∆H = -2600 kJ The energy released when 0.5 mole of each gas is mixed and ignited is A 260 kJ B 520 kJ C 650 kJ D 1300 kJ
You understand that energy is an extensible property. In other words the amount is proportional to the number of moles reacting?
Hi That is quite tricky- it's all about identifyimg which reagent is in excess- the C2H2 in this case-there isn't enough oxygen to react with it all. See attachment for worked answer
Hi That is quite tricky- it's all about identifyimg which reagent is in excess- the C2H2 in this case-there isn't enough oxygen to react with it all. See attachment for worked answer
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