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rainbow7020
26.08.2019 •
Chemistry
A24.0 g sample of nitrogen gas reacts with an excess of hydrogen gas to give an actual yield of 3.85 g nh3. what is the percent yield for this reaction given the reaction: n2(
g. 3h2(
g. --> 2nh3(g
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Ответ:
6.62%
Explanation:
We have the following reaction
A real yield of 3.85 g of
is obtained
To calculate the reaction yield in percentage we must calculate the mass that theoretically we must obtain
The reaction occurs in excess of hydrogen and 24.0g of N this means that when the nitrogen is finished the reaction will end
Nitrogen is our limit reagent
Molar mass of nitrogen![14 g/mol](/tpl/images/0199/0792/8b116.png)
This means that in 1 mol of nitrogen there is 14 g.
To calculate the moles of nitrogen in 24 g N we apply a simple rule of three
According to stoichiometric coefficients 1 mol of N produces 2 moles of![NH_3](/tpl/images/0199/0792/b033f.png)
1.71 mol N how many moles of
will produce
Molar mass of
17 g / mol
This means that in 1 mol of
there are 17 g.
58.14g
corresponds to the theoretical yield of the reaction
To calculate the percentage yield of the reaction we use the following formula
The percent yield for this reaction is 6.62%
Ответ:
He ripped his other suit