The equilibrium constant, K, for the reaction N204(9) = 2 NO2(g)
at 25°C is 5.88 x 10-3. Suppose 15.6 g of N204 is placed in a 5.00 L flask at 25°C. Calculate:
(a) The number of moles of NO2 present at equilibrium
(b) The percentage of the original N20, that is dissociated

0.66y = 0.9x + 0.48 if y has a value of 108.45 what is the value of x?

Ase your answer to this question on the information below.hydrocarbons and fissionable nuclei are among the sources used for the production of energy in the united states. a chemical reaction produces much less energy than a nuclear reaction per mole of reactant.the balanced chemical equation below represents the reaction of one molecule of a hydrocarbon with two molecules of oxygen.chemical equation: ch4 + 2o2 → co2 + 2h2o + 1.48 × 10−18 jthe nuclear equation below represents one of the many possible reactions for one fissionable nucleus. in this equation, x represents a missing product.nuclear equation: write an isotopic notation for the missing product represented by x in the nuclear equation.

In which environment would primary succession occur? a forest with a few remaining trees after a recent wildfire an area of exposed rock after a glacier melts away beach that is exposed to the air at low tide an abandoned baseball field in a small town