Chemistry, 18.03.2020 23:01 AlwaysMarcus5577
For the reaction 2 H2O(g) equilibrium reaction arrow 2 H2(g) + O2(g), K = 2.4 ✕ 10−3 at a given temperature. At equilibrium in a 2.7 L container, it is found that [H2O(g)] = 2.0 ✕ 10−1 M and [H2(g)] = 2.5 ✕ 10−2 M. Calculate the moles of O2(g) present under these conditions.
Answers: 1
moles of 
will be produced.
will be as follows,![K_{c} = \frac{[H_{2} ]^2[O_{2} ]}{[H_{2}O ]^2 }](/tpl/images/0552/7877/22d2b.png)
![2.4\times10^{-2} = \frac{[2.5\times10^{-2} ]^2[O_{2} ]}{[2\times10^{-1} ]^2 }](/tpl/images/0552/7877/022e7.png)
![[O_{2} ]=\frac{[2.4\times10^{-3}][2\times10^{-1} ]^2 }{[2.5\times10^{-2} ]^2}](/tpl/images/0552/7877/7587e.png)
![[O_{2}]= 1.5\times10^{-1}M](/tpl/images/0552/7877/aba91.png)
![[O_{2} ]= \frac{moles}{LItre}](/tpl/images/0552/7877/7e5ff.png)
![[1.5\times10^{-1} ]= \frac{moles}{2.7}](/tpl/images/0552/7877/f2d4f.png)
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For the reaction 2 H2O(g) equilibrium reaction arrow 2 H2(g) + O2(g), K = 2.4 ✕ 10−3 at a given temp...
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