What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?C(s) + 2 H2(g) ⇌ CH4(g) ∆H = -18 kcal/mol (-75kJ/mol)Increasing pressure by decreasing volume

Verified step by step guidance

1. Identify the reaction type: The given reaction is an equilibrium reaction involving gases, where carbon reacts with hydrogen to form methane.
2. Understand Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
3. Analyze the effect of pressure change: Increasing pressure by decreasing volume affects gaseous equilibria. The system will shift towards the side with fewer moles of gas to reduce pressure.
4. Count the moles of gas on each side: On the left side, there are 2 moles of H2 gas, and on the right side, there is 1 mole of CH4 gas.
5. Determine the shift in equilibrium: Since the right side has fewer moles of gas, the equilibrium will shift towards the formation of CH4 to decrease the pressure.

Key Concepts

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In the context of the given reaction, increasing pressure by decreasing volume will shift the equilibrium position towards the side with fewer gas molecules, which is essential for predicting the effect of pressure changes.

Equilibrium Position

The equilibrium position of a reaction refers to the relative concentrations of reactants and products at equilibrium. In the reaction C(s) + 2 H2(g) ⇌ CH4(g), the position can be influenced by changes in pressure, temperature, and concentration. Understanding how these factors affect the equilibrium position is crucial for analyzing the impact of pressure changes on the reaction.

Gas Laws

Gas laws describe the behavior of gases in relation to pressure, volume, and temperature. According to Boyle's Law, decreasing the volume of a gas at constant temperature increases its pressure. This principle is relevant when considering how changes in volume affect the equilibrium of gaseous reactions, such as the one involving hydrogen and methane in the given reaction.