The rapid decomposition of sodium azide, nan3, to its elements is one of the reactions used to inflate airbags: 2 nan3 (s)  2 na (s) + 3 n2 (g) how many grams of n2 are produced from 6.00 g of nan

The amount of nitrogen gas produced is 3.864 grams

Explanation:

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

    .....(1)

Given mass of = 6.00 g

Molar mass of = 65 g/mol

Putting values in equation 1, we get:

For the given chemical reaction:

By Stoichiometry of the reaction:

2 moles of produces 3 moles of nitrogen gas

So, 0.092 moles of will produce = of nitrogen gas

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

Molar mass of nitrogen gas = 28 g/mol

Moles of nitrogen gas = 0.138 moles

Putting values in equation 1, we get:

Hence, the amount of nitrogen gas produced is 3.864 grams

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.