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Paul [167]
3 years ago
14

A sample of 8.5 g nh3 on oxidation produces 4.5 g of no. calculate the percent yield. reaction: 4 nh3 5 o2 → 4 no 6 h2o

Chemistry
1 answer:
AnnZ [28]3 years ago
5 0
<span>30.% Determine the molar mass of NH3 and NO Atomic weight nitrogen = 14.0067 Atomic weight hydrogen = 1.00794 Atomic weight oxygen = 15.999 Molar mass NH3 = 14.0067 + 3 * 1.00794 = 17.03052 g/mol Molar mass NO = 14.0067 + 15.999 = 30.0057 g/mol Moles NH3 = 8.5 / 17.03052 = 0.499103962 mol Moles NO = 4.5 / 30.0057 = 0.149971505 mol Looking at the balanced equation, for every mole of NH3 consumed, you should get one mole of NO. So if we had 100% yield, we should have 0.499103962 moles of NO. But we don't. The percent yield is a simple matter of division by what we did get by what we should get. So 0.149971505 / 0.499103962 = 0.300481497 = 30.0481497% Rounding to 2 significant figures gives 30.% yield.</span>
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PLSSS HELP FAST
Aliun [14]

Note the formula

\boxed{\sf Mass\:no=No\:of\:protons+No\:of\:neutrons}

For X:-

  • No of protons:-

\\ \sf\longmapsto 19-10=9protons

  • It is Fluorine.

For Y:-

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\\ \sf\longmapsto 16-8=8protons

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Option D is correct

7 0
2 years ago
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Korvikt [17]

Answer:

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If the reaction is exothermic, its the vice versa

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