Given the following reaction and its equilibrium constant at a certain temperature, n2(g) + 3h2(g) ⇌ 2nh3(g) kc= 3.6x10^8
calculate the numerical value of the equilibrium constant for the following reaction at the same temperature.
nh3(g) ⇌ 1/2 n2(g) + 3/2 h2 (g) show work.
Answers: 3
![K'c=\frac{[N_{2}]^{1/2}.[H_{2}]^{3/2} }{[NH_{3}]}](/tpl/images/0383/7246/30b88.png)
![Kc=\frac{[NH_{3}]^{2} }{[N_{2}].[H_{2}]^{3} } =\frac{[NH_{3}].[NH_{3}]}{[N_{2}]^{1/2}.[N_{2}]^{1/2}. [H_{2}]^{3/2}.[H_{2}]^{3/2}} =(\frac{[NH_{3}]}{[N_{2}]^{1/2}.[H_{2}]^{3/2}} )^{2} =\frac{1}{K'c^{2} } \\K'c=\sqrt{\frac{1}{kc} } =\sqrt{\frac{1}{3.6 \times 10^{8} } } =5.3 \times 10^{-5}](/tpl/images/0383/7246/41914.png)
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Given the following reaction and its equilibrium constant at a certain temperature, n2(g) + 3h2(g) ⇌...
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