Consider the following equilibrium:
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Dinitrogen tetroxide decomposes to nitrogen dioxide N2O4 (g)--> 2NO2 (g). Delta H =55.3kJ. At 298K a reaction vessel contains 0.100 atm of N2O4. When equilibrium is reached 58% of the N2O4 has decomppsed to NO2 What percentage of N2O4 decomposes at 380 K ? Assume that the initial pressure of N2O4 is the same (0.100 atm).
At high temperatures, dinitrogen tetroxide gas decomposes to nitrogen dioxide gas. At 500 oC, a sealed vessel containing some dinitrogen tetroxide gas was allowed to reach equilibrium. At equilibrium, the mixture contained 3.64 M dinitrogen tetroxide gas. Calculate the equilibrium concentration of nitrogen dioxide if KC at this temperature is 0.715.
Provide your answer to two places after the decimal and without units.
Suppose a 500.mL flask is filled with 0.6mol of NO and 1.4mol of NO2. The following reaction becomes possible: NO3g + NOg <-->2NO2g The equilibrium constant K for this reaction is 0.506 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. *** must calculate for M first by dividing the moles by Liters before placing in the ICE table.