Question:

For a reaction, N2O5(g)2NO2(g)+12O2(g) {N}_2{O}_5(g) \rightarrow 2{NO}_2(g) + \frac{1}{2} {O}_2(g) in a constant volume container, no products were present initially. The final pressure of the system when 50% of the reaction gets completed is:

Show Hint

For reactions occurring in a constant volume container, use stoichiometry to calculate the total pressure by considering the moles of reactants and products formed at each step.
Updated On: Mar 17, 2025
  • 72 \frac{7}{2} times of initial pressure
  • 5 times of initial pressure
  • 52 \frac{5}{2} times of initial pressure
  • 74 \frac{7}{4} times of initial pressure
Hide Solution
collegedunia
Verified By Collegedunia

The Correct Option is D

Solution and Explanation

Let the initial pressure of N2O5 N_2O_5 be P0 P_0 .
At 50% reaction completion:
- 12P0 \frac{1}{2} P_0 of N2O5 N_2O_5 decomposes.
- This produces:
    - P0 P_0 of NO2 NO_2 ,
     - P04 \frac{P_0}{4} of O2 O_2 .
Thus, the total final pressure is: Pfinal=P02+P0+P04=7P04 P_{\text{final}} = \frac{P_0}{2} + P_0 + \frac{P_0}{4} = \frac{7P_0}{4} Hence, the final pressure is 74 \frac{7}{4} of the initial pressure.
Thus, the correct answer is: (4) \boxed{(4)} .
Was this answer helpful?
0
0

Top Questions on Chemical Reactions

View More Questions

Questions Asked in JEE Main exam

View More Questions