How much heat is evolved if 25.00 g of methanol (CH3OH) is burned in excess O2?
The reaction is:
2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(g) ΔH= -1453kJ

Question

How much heat is evolved if 25.00 g of methanol (CH3OH) is burned in excess O2?
The reaction is:
2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(g)    ΔH= -1453kJ

sweetburger · Answer

say that only 1 mole of Methanol was burned then the Delta H = -1453/2

so if we burn 25g of methanol and we convert grams of methanol to moles of methanol it is 25gmethanol/32gmethanol = .78125 so we multiprly .78125(-1453/2)

sweetburger · Answer

Does this explanation make sense?

anonymous · Answer

Yes it makes more sense now

anonymous · Answer

Is the answer -567.578 kJ?

sweetburger · Answer

ya

anonymous · Answer

thanks dude can you help me with some more?