What is the limiting reagent when 49.84 g of nitrogen react with 10.7 g of hydrogen according to this balanced equation: n2(g) 3h2(g) → 2nh3(g) ?

The limiting reagent for the given chemical reaction is hydrogen.

Explanation:

To calculate the number of moles, we use the equation:

  .....(1)

Given mass of nitrogen = 49.84 g

Molar mass of nitrogen = 28 g/mol

Putting values in above equation, we get:

Given mass of hydrogen = 10.7 g

Molar mass of hydrogen = 2 g/mol

Putting values in above equation, we get:

For the given chemical reaction:

By Stoichiometry of the reaction:

3 moles of hydrogen reacts with 1 mole of nitrogen.

So, 5.32 moles of hydrogen reacts with = of nitrogen.

As, the given amount of nitrogen is more than the required amount, so it is considered as an excess reagent.

Thus, hydrogen is considered as an limiting reagent because it limits the formation of products.

Hence, the limiting reagent for the given chemical reaction is hydrogen.

d: the voltage of the secondary coil is less than that of the primary coil.

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