Nitrogen dioxide is introduced in to a flask at a pressure of one atmosphere (1.00atm). after some time it dimerizes to produce n2o4. a) what is the equilibrium partial pressure of n2o4 at a temperature where the equilibrium constant for dimerization is kc=3.33?

h let me think

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

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i think? ?

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.