Question

s PCl_3 + Cl_2" alt="PCl_5 \rightleftarrows PCl_3 + Cl_2" align="absmiddle" class="latex-formula">PCl₅ (g) decomposes into PCl₃ (g) and Cl₂ (g) according to the equation above. A pure sample of PCl₅ (g) is placed in a rigid, evacuated 1.00 L container. The initial pressure of the PCl₅ (g) is 1.00 atm. The temperature is held constant until the PCl₅ (g) reaches equilibrium with its decomposition products.If the decomposition reaction were to go to completion, the total pressure in the container will be:(A) 1.4 atm(B) 2.0 atm(C) 2.8 atm(D) 3.0 atm

Answer 1

Answer: The total pressure of the container will be 2.00 atm

Explanation:

We are given:

Initial moles of phosphorus pentachloride = 1.00 atm

For the given chemical reaction:

$PCl_5\rightleftharpoons PCl_3+Cl_2$

By Stoichiometry of the reaction:

1 mole of $PCl_5$ produces 1 mole of $PCl_3$ and 1 mole of chlorine gas

So, 1.00 atm of $PCl_5$ will also produce 1.00 atm of $PCl_3$ and 1.00 atm of chlorine gas when the reaction goes to completion.

Total pressure of the container when the reaction goes to completion  = 1.00 + 1.00 = 2.00 atm

Hence, the total pressure of the container will be 2.00 atm