Question

The following reaction occurs when a burner on a gas stove is lit:

CH4(g) + 2O2(g) ⇄ CO2(g) + 2H20(g)


Evaluate the following statements and select the correct grouping. True statements are marked with a T, and false statements are marked with an F.


The system cannot reach equilibrium because it is not a closed system.

Increasing the concentration of the CH4 will increase the production of CO2 and water.

Increasing the temperature of the flame will increase the production of CO2 and water.

Adding CO2 will increase the volume of methane and oxygen

Answer 1

The correct grouping is:

F, T, T, F

Step-by-step explanation:

- The first statement is false. Although the system is not closed in the strictest sense, it can still reach equilibrium because the reactants and products are all gases and can interact with each other.
- The second statement is true. According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium towards the products, in this case, CO2 and water.
- The third statement is also true. Increasing the temperature will increase the rate of the forward reaction, causing the equilibrium to shift towards the products.
- The fourth statement is false. Adding CO2 to the system will not affect the volume of methane and oxygen. It may, however, affect the equilibrium position by shifting it towards the reactants, as Le Chatelier's principle predicts that adding a product will shift the equilibrium towards the reactants.