Answer:
[tex]p_f=0.5atm[/tex]
Explanation:
Hello!
In this case, since the reaction between nitrogen and hydrogen produces ammonia:
[tex]N_2+3H_2\rightarrow 2NH_3[/tex]
We can compute the volume of the container by using the ideal gas law at STP (1 atm and 273.15 K):
[tex]V=\frac{4.0mol*0.08206\frac{atm*L}{mol*K}*273.15K}{1atm}=89.7L[/tex]
Next, since nitrogen and hydrogen are in a 1:3 mole ratio, we understand all the nitrogen and hydrogen are consumed and only ammonia remains at the end of the reaction in the following amount:
[tex]n_{NH_3}=1.0molN_2*\frac{2molNH_3}{1molN_2} =2.0molNH_3[/tex]
Thus, the final pressure turns out:
[tex]p_f=\frac{2.0mol*0.08206\frac{atm*L}{mol*K}*273.15K}{89.7L}\\\\p_f=0.5atm[/tex]
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