(1) According to the data in the table, the stoichiometric ratio of C, NO, E and F is 0.15: 0.3: 0.15 =1:2: 65438+. N2+CO2, because it is uncertain whether the positive reaction is endothermic or exothermic, it is impossible to judge the temperature change.

So the answer is: C+2NO? N2+ CO2; Not sure;

(2) When the catalyst is added, the forward and reverse reaction rates should be increased to the same extent, and the ordinate of the image is the rate, which should be increased when the catalyst is added.

So, the answer is: incorrect; When a catalyst is used, the forward and reverse reaction rates should be increased to the same extent and higher than when there is no catalyst.

(3) the ionic equation of the reaction is ionic equation: SrSO4(s)+CO32-(aq)? SrCO3(s)+SO42-(aq), and the equilibrium constant is K=[SO42? 】【CO32？ ], the equilibrium constant is only affected by temperature. With the increase of ion concentration, the equilibrium constant remains unchanged, so the answer is: K=[SO42? 】【CO32？ ]; Constant;

(4) Because the equilibrium constant of H2CO3 is Ka1> Ka2 of H2SO4 > Ka2 of H2CO3, and the acidity of H2CO3 is > HSO3-> HCO3-, a sufficient amount of NaHSO3 solution is added into Na2CO3 solution to react to generate SO32- and HCO3-, and the ionic equation of the reaction is HSO3-+CO32-= SO32-+.

So the answer is: HSO3-+CO32-= SO32-+HCO3-; According to the ionization equilibrium constant, the acidity is H2CO3 > HSO3- > HCO3-, so HSO3- reacts with CO32- to generate SO32- and HCO3-, which cannot release carbon dioxide.