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

Answer : The correct option is, (I)

Solution : Given,

Mass of NO = 45.8 g

Mass of = 12.4 g

Molar mass of NO = 30 g/mole

Molar mass of = 2 g/mole

Molar mass of = 17 g/mole

First we have to calculate the moles of NO and .

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 2 mole of react with 5 mole of

So, 1.53 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of

From the reaction, we conclude that

As, 2 mole of react to give 2 mole of

So, 1.53 mole of react to give 1.53 mole of

Now we have to calculate the mass of

Therefore, the maximum mass of produced 26.0 grams.

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