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Post by ehela on Nov 7, 2016 22:52:59 GMT -5
Calculate the number of grams of H2(g) that are required to react with 1.25 x 10^27 molecules of N2(g)
I'm lost and i got a test tomorrow lol help me plz
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Post by ehela on Nov 7, 2016 22:57:44 GMT -5
ok I got 4.56*10^51 gram H2 is this correct
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Post by tiger beetle on Nov 7, 2016 23:09:57 GMT -5
uh okay so the reaction should be something like
3H2 + N2 = 2NH3
1.25*10^27 / 6.022*10^23 = moles of N2
3 * moles of N2 = moles of H2
moles of H2 * 2.02 = g of H2
3 * 2.02 * 1.25*10^27 / 6.022*10^23 = answer
assuming I did it correctly, that would be 75750 g H2, but maybe don't trust me?
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Post by ehela on Nov 7, 2016 23:11:09 GMT -5
aahh ok i multiplied by 6.022 instead of divided my bad, thanks so much!! thats it for now, but in five min i might come back with another question lol
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Post by tiger beetle on Nov 7, 2016 23:12:25 GMT -5
aahh ok i multiplied by 6.022 instead of divided my bad, thanks so much!! thats it for now, but in five min i might come back with another question lol you're welcome!
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