A. Comparing experiments ① and ②, the concentration of reactant A is the same when reaching equilibrium, so the equilibrium constant is the same, so A is wrong;

B. When the reaction rate increases, it may be to increase the temperature or pressure, but if the pressure increases, the volume of the container decreases, but the equilibrium concentration of A increases instead, which is not in line with the image and should be to increase the temperature. Because the temperature rises, the chemical equilibrium moves to the endothermic direction, and the concentration of A decreases at equilibrium, which shows that the positive reaction direction absorbs heat, so B is correct;

C. according to? A+2B？ C

Initial (mol/L)? 0. 1 0.20

Conversion (mol/L) 0.04 0.08? 0.04

Equilibrium (mole/liter)? 0.06 0. 12? 0.04

So the conversion rate of B at equilibrium is 0.080.2=0.4, so C is wrong;

D. according to? A+2B？ C

Initial (mol/L)? 0. 1 0.20

Conversion (mol/L) 0.060. 12? 0.06

Equilibrium (mole/liter)? 0.040.08 0.06?

So the concentration of C is 0.06mol/L at equilibrium, so D is wrong.

So choose B.