For the decomposition of the compound,

Question:

For the decomposition of the compound, represented as

$\mathrm{NH}_{2} \mathrm{COONH}_{4}(\mathrm{~s}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{CO}_{2}(\mathrm{~g})$

the $\mathrm{K}_{\mathrm{P}}=2.9 \times 10^{-5} \mathrm{~atm}^{3}$.

If the reaction is started with $1 \mathrm{~mol}$ of the compound, the total pressure at equilibrium would be

  1. $38.8 \times 10^{-2} \mathrm{~atm}$

  2. $1.94 \times 10^{-2} \mathrm{~atm}$

  3. $5.82 \times 10^{-2} \mathrm{~atm}$

  4. $7.66 \times 10^{-2} \mathrm{~atm}$


Correct Option: , 3

Solution:

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