Question

In the equilibrium system below, which of the following changes would cause the equilibrium position to shift to the right?

CO(g) + 3H2 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. CH4 (g) + H2O (g) delta H = -206 kJ/mol (2 points)

decreasing the concentration of carbon monoxide (CO)

increasing the volume of the reaction system

decreasing the concentration of hydrogen gas (H2)

lowering the temperature of the reaction

Answer 1

We are given with the equation that produces methane and water from the raection of hydrogen gas and carbon monoxide. This is expressed in the balanced equation: 3H2 + CO = CH4 + H2O. This is an exothermic process. THE CHANGE THAT IS OCCURING IS LOWERING THE TEMPERATURE OF THE MINIMAL REACTION

Answer 2

lowering the temperature of the reaction

Step-by-step explanation:

According to Le Chatelier's principle, when a system at equilibrium is subject to changes in temperature, pressure or concentration then the equilibrium will shift in a direction so as to undo the effect of the induced change.

The given reaction is:

`CO(g) + 3H2(g)\rightleftharpoons CH4(g) + H2O(g)`

ΔH = -206 kJ/mol.

Since the enthalpy change is negative, heat is evolved and the reaction is exothermic. Therefore, if the temperature of the reaction is lowered then it will shift the equilibrium in a direction of higher temperature i.e. towards evolution of heat. This will shift it to the right.