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The chemical equation for the synthesis of ammonia is as follows. nitrogen hydrogen ammonia N_(2(g))+3H_(2(g))arrow 2NH_(3(g)) Kevin needs to determine how many liters of nitrogen are needed to form 6 moles of ammonia. He sets up his stoichiometry equation like this: (6molNH_(3))/(1)times (2molN_(2))/(1molNH_(3))times (22.4LN_(2))/(1molN_(2))=268.8LN_(2) What error did Kevin make in his stoichiometry setup? Kevin should have multiplied moles of NH_(3) by the correct mole ratio of (2molN_(2))/(2molNH_(3)) instead of multiplying by (2molN_(2))/(1molNH_(3)) B Kevin should have multiplied moles of NH_(3) by the correct mole ratio of (1molN_(2))/(2molNH_(3)) instead of multiplying by (2molN_(2))/(1molNH_(3)) C Kevin should have started with the starting units of liters of N_(2) to determine the moles of NH_(3) needed. D Kevin should have converted from moles of NH_(3) to liters of NH_(3) fore multiplying by the mole ratio.

Pergunta

The chemical equation for the synthesis of ammonia is as follows.
nitrogen hydrogen
ammonia
N_(2(g))+3H_(2(g))arrow 2NH_(3(g))
Kevin needs to determine how many liters of nitrogen are needed to form 6
moles of ammonia. He sets up his stoichiometry equation like this:
(6molNH_(3))/(1)times (2molN_(2))/(1molNH_(3))times (22.4LN_(2))/(1molN_(2))=268.8LN_(2)
What error did Kevin make in his stoichiometry setup?
Kevin should have multiplied moles of NH_(3)
by the correct mole ratio
of
(2molN_(2))/(2molNH_(3))
instead of multiplying by
(2molN_(2))/(1molNH_(3))
B
Kevin should have multiplied moles of NH_(3) by the correct mole ratio
of
(1molN_(2))/(2molNH_(3))
instead of multiplying by
(2molN_(2))/(1molNH_(3))
C
Kevin should have started with the starting units of liters of N_(2) to
determine the moles of NH_(3) needed.
D
Kevin should have converted from moles of NH_(3) to liters of NH_(3)
fore multiplying by the mole ratio.

The chemical equation for the synthesis of ammonia is as follows. nitrogen hydrogen ammonia N_(2(g))+3H_(2(g))arrow 2NH_(3(g)) Kevin needs to determine how many liters of nitrogen are needed to form 6 moles of ammonia. He sets up his stoichiometry equation like this: (6molNH_(3))/(1)times (2molN_(2))/(1molNH_(3))times (22.4LN_(2))/(1molN_(2))=268.8LN_(2) What error did Kevin make in his stoichiometry setup? Kevin should have multiplied moles of NH_(3) by the correct mole ratio of (2molN_(2))/(2molNH_(3)) instead of multiplying by (2molN_(2))/(1molNH_(3)) B Kevin should have multiplied moles of NH_(3) by the correct mole ratio of (1molN_(2))/(2molNH_(3)) instead of multiplying by (2molN_(2))/(1molNH_(3)) C Kevin should have started with the starting units of liters of N_(2) to determine the moles of NH_(3) needed. D Kevin should have converted from moles of NH_(3) to liters of NH_(3) fore multiplying by the mole ratio.

Solução

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PietraMestre · Tutor por 5 anos

Responder

The correct answer is B. Kevin should have multiplied moles of NH_{3}
by the correct mole ratio of \frac {1molN_{2}}{2molNH_{3}}
instead of multiplying by \frac {2molN_{2}}{1molNH_{3}}
.
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