<p>Heheh, such an easy test :D</p>
<p>It was like 70 something for that one</p>
<p>i remember it being like 140’s ish…maybe a different one though?</p>
<p>ha, maybe 140 was what it was given then.</p>
<p>It can’t be 140 - that’s what you get per 2 moles of H20, it asked for 1 mole of H2O so you divide by 2</p>
<p>couldn’t it be 1/4 of the energy because of the stoichiometry
just 1/2 seems too easy</p>
<p>i got whatever the gave you/2. is that 70?</p>
<p>did it say the delta Hf of 1 mol of water is 140, given this unbalanced (or was it balanced, or was there no equation) how much energy is there</p>
<p>i remember it asking the question dealing with moles of H2 or O2 not with H2O?</p>
<p>i put half of whatever they gave…</p>
<p>If you did half that’s energy per 2 moles - it’s half divided by 2 =P</p>
<p>Yeah, I’m pretty sure that ~-140 is the answer.</p>
<p>It said that dHformation for H2O is -285 (1 mole water). Then it asked for what dH would be if .5 moles were formed.</p>
<p>-285 kJ/1 mol H2O * .5 moles H2O = ~-140 kJ</p>
<p>so it is 1/4</p>
<p>1/4 of the ACTUAL value for the equation, but 1/2 of the value they gave you, I think.</p>
<p>(Haha I don’t even remember the question but I know I got it right =P)</p>
<p>^ exactly LOL. so confusing.</p>
<p>so was it 70?</p>
<p>I don’t think so. It gave you -285 kJ/ 1 mol H2O, then asked what dH was when .5 mols reacted.</p>
<p>No, what you’re thinking of is dH per RXN. The value given was per ONE MOLE of H2O (not per 2 moles, like in the actual reaction).</p>
<p>Eloquence and i put 70
Eloquence do u think u did it right?</p>
<p>i got 140 also.</p>
<p>What was the heat of formation they gave us?</p>
<p>Which was most difficult to oxidize? choices were F2, H2, C, and 2 other metals. I put F2 - anyone agree?</p>
<p>140 .</p>