Question

Phosphorus pentachloride decomposes according to the following equation. $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$ $K_c = 0.0150$ What are the concentrations (in M) of $PCl_5$, $PCl_3$, and $Cl_2$ in an equilibrium mixture produced by the decomposition of a sample of pure $PCl_5$ with an initial $[PCl_5]$ of 1.82 M? Hint: you will need the quadratic formula or method of successive approximations (see Appendix A1.4 for review if needed). $[PCl_5] = 1.834$ M $[PCl_3] = 0.166$ M $[Cl_2] = 0.166$ M

          Phosphorus pentachloride decomposes according to the following equation.
$PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$
$K_c = 0.0150$
What are the concentrations (in M) of $PCl_5$, $PCl_3$, and $Cl_2$ in an equilibrium mixture produced by the decomposition of a sample of pure $PCl_5$ with an initial $[PCl_5]$ of 1.82 M?
Hint: you will need the quadratic formula or method of successive approximations (see Appendix A1.4 for review if needed).
$[PCl_5] = 1.834$ M
$[PCl_3] = 0.166$ M
$[Cl_2] = 0.166$ M

Phosphorus pentachloride decomposes according to the following equation.
PCl5(g) ⇌ PCl3(g) + Cl2(g)
Kc = 0.0150
What are the concentrations (in M) of PCl5, PCl3, and Cl2 in an equilibrium mixture produced by the decomposition of a sample of pure PCl5 with an initial [PCl5] of 1.82 M?
Hint: you will need the quadratic formula or method of successive approximations (see Appendix A1.4 for review if needed).
[PCl5] = 1.834 M
[PCl3] = 0.166 M
[Cl2] = 0.166 M

Added by Sarah P.

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