I don't get the $ signs or the $$ signs. Nor do I see a question. I presume that the question is to determine the equilibrium concentrations after the SO2 concentration is changed form 0.300 to 0.800. Here is how you do that. I will delete the $ signs and balance the equation.
.................NO2(g)+SO2(g) ==> NO(g)+SO3(g)
E...............0.100.......0.300...........2.00......0.600
[NO2] = 0.100 M,
First determine Kc. Plug those equilibrium numbers as shown into Kc expression as shown here. Kc = (NO)(SO3)/(NO2)(SO2)
Kc = (2.00)(0.600)/(0.100)(0.300) = 40
Next we redo the equation to show the new concentrations at THE NEW CONDITIONS AS INITIAL and finish the ICE chart.
.................NO2(g)+SO2(g) ==> NO(g)+SO3(g)
I...............0.100.......0.800...........2.00......0.600
C...................-x..........-x................+x...........+x
E...............0.100-x....0.800-x.......2.00+x......0.600+x
Now plug the E line into the Kc expression and solve for x, then evaluate each of the reactants and products concentrations.
Post your work if you get stuck.
Nitrogen dioxide reacts with SO2 to form NO and SO3:
$$NO2(g)+SO2(g)
NO(g)+SO3(g)
An equilibrium mixture is analyzed at a certain temperature and found to contain [NO2] = 0.100 M,
[SO2] = 0.300 M, [NO] = 2.00 M, and [SO3] = 0.600 M. At the same temperature, extra SO2(g) is added to make a total [SO2] = 0.800 M.
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