Given the following chemical equation, determine how many grams of n2 are produced by 9.24 of h2o2 nd 6.56g of n2h4?

The mass of nitrogen gas produces is 3.81 grams.

Explanation:

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

     .....(1)

For hydrazine:

Given mass of hydrazine = 6.56 g

Molar mass of hydrazine = 32.0 g/mol

Putting values in equation 1, we get:

For hydrogen peroxide:

Given mass of hydrogen peroxide = 9.24 g

Molar mass of hydrogen peroxide = 34.0 g/mol

Putting values in equation 1, we get:

The chemical equation for the reaction of hydrazine and hydrogen peroxide follows:

By Stoichiometry of the reaction:

2 moles of hydrogen peroxide reacts with 1 mole of hydrazine

So, 0.272 moles of hydrogen peroxide will react with = of hydrazine

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

Thus, hydrogen peroxide is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of hydrogen peroxide produces 1 mole of nitrogen gas

So, 0.272 moles of hydrogen peroxide will produce = of nitrogen gas

Now, calculating the mass of nitrogen gas by using equation 1, we get:

Molar mass of nitrogen gas = 28.0 g/mol

Moles of nitrogen gas = 0.136 moles

Putting values in equation 1, we get:

Hence, the mass of nitrogen gas produces is 3.81 grams.

What are the choices?

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