The equilibrium constant for the thermal decomposition of NO2 is 7.32 10-6 at 450 K. If a reaction vessel at this temperature initially contains 0.515 atm of NO2, what will the partial pressures of NO2, NO, and O2 be when equilibrium has been established? Since Kp is small, you can use simplifying assumptions. Be sure not to round your numbers during the calculation and use at least 3 sig figs.

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The equilibrium constant for the thermal decomposition of NO2 is 7.32 10-6 at 450 K. If a reaction vessel at
this temperature initially contains 0.515 atm of NO2, what will the partial pressures of NO2, NO, and O2 be
when equilibrium has been established? Since Kp is small, you can use simplifying assumptions. Be sure not
to round your numbers during the calculation and use at least 3 sig figs.
Transcribed Image Text:The equilibrium constant for the thermal decomposition of NO2 is 7.32 10-6 at 450 K. If a reaction vessel at this temperature initially contains 0.515 atm of NO2, what will the partial pressures of NO2, NO, and O2 be when equilibrium has been established? Since Kp is small, you can use simplifying assumptions. Be sure not to round your numbers during the calculation and use at least 3 sig figs.
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