Question

# One mole of $$NH_{4}Cl(s)$$ is kept in an open container & then covered with a lid. The container is now heated up to $$600 K$$ where $$NH_{4}Cl(s)$$ completely dissociates into $$NH_{3}(g)$$ & $$HCl(g).$$ If a volume of the container is $$24.63$$ liters, calculate what will be the final pressure of the gases inside the container? Assume that outside air is at $$300 K$$ and 1 atm pressure.

A
0.5 atm;
B
2.5 atm;
C
1.5 atm;
D
None of these

Solution

## The correct option is D None of these$$\displaystyle \underset {\text {1 mol}}{NH_4Cl(s)} \rightleftharpoons \underset {\text {1 mol}}{NH_3(g)} +\underset {\text {1 mol}}{HCl(g)}$$$$\displaystyle P = \frac {nRT}{V} = \frac {2 \times 0.0821 \times 600}{24.63} = 4 \: atm$$Thus, the total pressure of gases inside container is 4 atm.Chemistry

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