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Veseljchak [2.6K]
3 years ago
14

if 75 moles of ammonia is needed, how many grams of nitrogen will be consumed? N2(g) + 3H2(g) --> 2NH3(g)

Chemistry
2 answers:
Hatshy [7]3 years ago
7 0

Answer:

Amount of nitrogen consumed comes out to be 1050 g

Explanation:

Number of moles of ammonia needed = 75 mole

The balanced reaction is shown below

\textrm{N}_{2}\left ( g \right )+3\textrm{H}_{2}\left ( g \right )\rightarrow 2\textrm{NH}_{3}\left ( g \right )

1 mole of ammonia is needed for producing 2 mole ammonia according to the balanced reaction.

Number of moles of nitrogen needed for producing 75 mole ammonia = 37.5 mole

Molar mass of nitrogen gas = 28 g/mole

Amount of nitrogen gas needed = \left ( 37.5 \textrm{ mole}\times 28 \textrm{ g/mol} \right ) = 1050 \textrm{ g}

Amount of nitrogen gas needed = 1050 g

zalisa [80]3 years ago
3 0

Answer: 37.5

Explanation: Since NH3 has a coefficient of 2, that means it will produce 2x the moles as N2. Since 75 moles of NH3 will be used, in order to figure out N2 you would do the following:

75 mol / 2 = 37.5

Oh wait this said grams, sorry! Let me fix it.

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Explanation:

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Determine the number of grams of sodium carbonate needed to prepare 100.0 ml of a 2.5 m solution
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First we convert 100.0 mL to L:

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Now we <u>calculate how many moles of sodium carbonate are needed</u>, using the <em>definition of molarity</em>:

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Finally we <u>convert 0.25 moles of sodium carbonate into grams</u>, using its <em>molar mass</em>:

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