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zimovet [89]
3 years ago
12

Consider the following reaction: 2 NO(g) + 5 H2(g) → 2 NH3(g) + 2 H2O(g) Which set of solution maps would be needed to calculate

the maximum amount of ammonia (NH3), in grams, that can be synthesized from 45.8 g of nitrogen monoxide (NO) and 12.4 g of hydrogen (H2)? I. g NO → mol NO → mol NH3 → g NH3 II. g H2 → mol H2 → mol NH3 → g NH3 III. g NO → mol NO → mol H2O → g H2O IV. g H2 → mol H2 → mol H2O → g H2O
Chemistry
1 answer:
Leto [7]3 years ago
7 0

Answer : The correct option is, (I) gNO\rightarrow molNO\rightarrow molNH_3\rightarrow gNH_3

Solution : Given,

Mass of NO = 45.8 g

Mass of H_2 = 12.4 g

Molar mass of NO = 30 g/mole

Molar mass of H_2 = 2 g/mole

Molar mass of NH_3 = 17 g/mole

First we have to calculate the moles of NO and O_2.

\text{ Moles of }NO=\frac{\text{ Mass of }NO}{\text{ Molar mass of }NO}=\frac{45.8g}{30g/mole}=1.53moles

\text{ Moles of }H_2=\frac{\text{ Mass of }H_2}{\text{ Molar mass of }H_2}=\frac{12.4g}{2g/mole}=6.20moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

2NO(g)+5H_2(g)\rightarrow 2NH_3(g)+2H_2O(g)

From the balanced reaction we conclude that

As, 2 mole of NO react with 5 mole of H_2

So, 1.53 moles of NO react with \frac{1.53}{2}\times 5=3.82 moles of H_2

From this we conclude that, H_2 is an excess reagent because the given moles are greater than the required moles and NO is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of NH_3

From the reaction, we conclude that

As, 2 mole of NO react to give 2 mole of NH_3

So, 1.53 mole of NO react to give 1.53 mole of NH_3

Now we have to calculate the mass of NH_3

\text{ Mass of }NH_3=\text{ Moles of }NH_3\times \text{ Molar mass of }NH_3

\text{ Mass of }NH_3=(1.53moles)\times (17g/mole)=26.0g

Therefore, the maximum mass of NH_3 produced 26.0 grams.

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