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determine if the reaction is product-favored, reactant-favored, or at equilibrium.?
The reaction below has an equilibrium constant, K, of 171 at 25°C. Using the reaction conditions given, determine if the reaction is product-favored, reactant-favored, or at equilibrium.
2 NO2(g) D N2O4(g)
**(D represents the two arrows each pointing a different way)
2.0x10-3 mol NO2, 1.5x10-3 mol N2O4, 5.0 L flask
2 Answers
- pisgahchemistLv 71 decade agoFavorite Answer
2 NO2(g) <==> N2O4(g)
At 25C, the value of K indicates that the equilibrium lies farther to the right, with more N2O4 than NO2.
When roughly equal amounts of NO2 and N2O4 are combined at 25C, then the equilibrium concentration of N2O4 will be greater.
You can use an ICE table and do the math if you really want to determine the equilibrium concentrations.
================= Follow up ===================
Benjamin wrote, "... chemicaly it should be reactant favoured as N2O4 is unstable and would collapse back into its constituant state almost immediatly after bieng created...". (sic) This is nonsense.
- Anonymous1 decade ago
chemicaly it should be reactant favoured as N2O4 is unstable and would collapse back into its constituant state almost immediatly after bieng created :)
