Chemistry, 30.03.2020 17:28 natalie2sheffield
G Potassium chlorate decomposes to product potassium chloride and oxygen gas. 2KClO3(s) ⇔ 2KCl(s) + 3O2(g) When this reaction was run at room temperature, the following equilbrium concentrations were measured: [O2] = 0.0500 M; [KCl] = 0.00250 M; [KClO3] = 2.00 M What is the equilibrium constant for this reaction?
Answers: 3
is the equilibrium constant for this reaction.![[O_2] = 0.0500 M](/tpl/images/0570/5147/94139.png)
![[KCl] = 0.00250 M](/tpl/images/0570/5147/3a302.png)
![[KClO_3] = 2.00 M](/tpl/images/0570/5147/90bf6.png)
![K_c=\frac{[KCl]^2[O_2]^3}{[KClO_3]^2}](/tpl/images/0570/5147/bd160.png)
![=\frac{[0.00250 M]^2[0.0500 M]^3}{[2.00 M]^2}](/tpl/images/0570/5147/c5974.png)
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G Potassium chlorate decomposes to product potassium chloride and oxygen gas. 2KClO3(s) ⇔ 2KCl(s) +...
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