The correct option is B. To increase the production of ammonia, you have to increase the pressure of the system. Increase in pressure will result in increased production of ammonia because this will drive the chemical reaction forward.
When you have the bottom measurement of the triangle (base) and the height of the triangle in the center, you multiply them together and then divide by 2.
~Do you need more explaining~?
Based on Le Chatelier's principle, if a system at equilibrium is disturbed by changes in the temperature, pressure or concentration, then the equilibrium will shift in a direction to undo the effect of the induced change.
The given reaction is endothermic i.e, heat is supplied:
CH4(g) + H2O (g) + heat ↔ 3H2(g) + CO(g)
a) When the temperature is lowered, heat is being removed from the system. The reaction will move in a direction to produce more heat i.e. to the left.
Hence, the pressure of CH4 will increase and equilibrium will shift to the left
b) When the temperature is raised, heat is being added to the system. The reaction will move in a direction to consume the added heat i.e. to the right.
Hence, the pressure of CO will increase and equilibrium will shift to the right
