The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.PCl5(g) PCl3(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [PCl5] = M [PCl3] = M [Cl2] = M
The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.PCl5(g) PCl3(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [PCl5] = M [PCl3] = M [Cl2] = M
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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Question
The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.
PCl5(g) PCl3(g) + Cl2(g)
Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K.
| [PCl5] | = | M |
| [PCl3] | = | M |
| [Cl2] | = | M |
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