Chemistry Question Need Help! Heat?

Question

Please help me some school work am confuse about.

How much heat will be released when 6.44g of sulfur reacts with excess O2 according to the following equation?

2S + 3O2 ⇒ 2SO3 ΔH゜= -791.4kJ.

i was taught to solve it i need to do the following(not 100% sure if this is the right way to solve this)

6.44g x 1mol/32 x -791.4/2mol = the answer.

My question is. Is this the right way to solve it. and for the question if i replace the word "Released" to "absorbed" obviously　ΔH゜ would a positive number. if it's positive do I need a different way to solve it?

Answer 1

delta H is kj/mol

change 6.44 g S to mol SO2 using stoichiometry

(6.44 g S) x [(1 mol S / (32.1 g S)] x [(2 mol SO2) / (2 mol S)] = moles SO2

proportion: (-794.1 kj / 1 mol) = (unknown kj / mole answer above)

Answer 2

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Answer 3

It should be correct, the reason it stands in negative, is becaurse it looses energy to it´s surroundings, if it was a positive it would absorb energy.