- #1
crybllrd
- 120
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We just started learning this in chem, and I thought it was quite simple.
I missed the particular lecture, and am now paying the price:
The following chemical reaction has reached equilibrium:
2NO + O[tex]_{2}[/tex] [tex]\rightarrow[/tex]2NO[tex]_{2}[/tex]
Calculate the equilibrium constant (K[tex]_{eq}[/tex]) if the concentrations of reactants and products are 1.26 × 10[tex]^{-10}[/tex] M for NO, 2.28 × 10[tex]^{-3}[/tex] M for O[tex]_{2}[/tex], and 9.32 × 10[tex]^{-6}[/tex] M for NO[tex]_{2}[/tex].
K[tex]_{eq}[/tex]=[tex]\frac{products}{reactants}[/tex]
This is the equation I found, but what units do I use? Molar, mol, kg, ...
And how do coefficients play a role?
How do I proceed?
BTW I see my subscripts aren't correctly formatted, LATEX says it's correct, so I don't know how to fix it...
I missed the particular lecture, and am now paying the price:
The following chemical reaction has reached equilibrium:
2NO + O[tex]_{2}[/tex] [tex]\rightarrow[/tex]2NO[tex]_{2}[/tex]
Calculate the equilibrium constant (K[tex]_{eq}[/tex]) if the concentrations of reactants and products are 1.26 × 10[tex]^{-10}[/tex] M for NO, 2.28 × 10[tex]^{-3}[/tex] M for O[tex]_{2}[/tex], and 9.32 × 10[tex]^{-6}[/tex] M for NO[tex]_{2}[/tex].
K[tex]_{eq}[/tex]=[tex]\frac{products}{reactants}[/tex]
This is the equation I found, but what units do I use? Molar, mol, kg, ...
And how do coefficients play a role?
How do I proceed?
BTW I see my subscripts aren't correctly formatted, LATEX says it's correct, so I don't know how to fix it...
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