If 3.0 atm of pure HN3(g) is decomposed initially, what is the final total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.

This is an incomplete question, here is a complete question.

Hydrogen azide, HN₃, decomposes on heating by thefollowing unbalanced reaction:

If 3.0 atm of pure HN₃ (g) is decomposed initially,what is the final total pressure in the reaction container? Whatare the partial pressures of nitrogen and hydrogen gas? Assume thatthe volume and temperature of the reaction container are constant.

Answer : The partial pressure of and gases are, 4.5 atm and 1.5 atm respectively.

Explanation :

The given unbalanced chemical reaction is:

This reaction is an unbalanced chemical reaction because in this reaction number of hydrogen and nitrogen atoms are not balanced on both side of the reaction.

In order to balance the chemical equation, the coefficient '2' put before the and the coefficient '3' put before the then we get the balanced chemical equation.

The balanced chemical reaction will be,

As we are given:

The pressure of pure = 3.0 atm

From the reaction we conclude that:

Number of moles of = 3 mol

Number of moles of = 1 mol

Now we have to calculate the mole fraction of and

and,

Now we have to calculate the partial pressure of and

According to the Raoult's law,

where,

= partial pressure of gas

= total pressure of gas  = 6.0 atm

= mole fraction of gas

and,

Thus, the partial pressure of and gases are, 4.5 atm and 1.5 atm respectively.

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