Question

Hydrogen gas can be produced using this equilibrium reaction. Which change would drive this process toward the product side?

C +H20 =CO+ H2 + energy

A. Increasing the temperature.
B. Removing the H2O as it forms.
C. Removing the CO as it forms.
D. Removing the C as it forms.

Answer 1

To drive the reaction C + H2O = CO + H2 + energy toward the product side and produce more hydrogen gas, removing H2O or CO as they form would be effective strategies, based on Le Chatelier's Principle.Correct answer is option B.

Step-by-step explanation:

The student's question concerns the effect of different changes on the equilibrium of the reaction C + H2O = CO + H2 + energy. To drive the reaction toward the production of hydrogen gas (H2), one should make changes that favor the formation of products according to Le Chatelier's Principle. Given that the reaction is endothermic (energy is a product), increasing the temperature would indeed drive the reaction towards the right, increasing the formation of CO and H2.

However, options B, C, and D involve removing components from the reaction mixture. Removing H2O or CO as they form would also shift the equilibrium towards the product side to compensate for the change. Removing carbon (C) would not be effective as it is not a gas and its removal from the system might not have an immediate impact on the gas-phase equilibrium. Therefore, removing H2O or CO as they form (options B and C) would be effective ways to drive the reaction towards producing more products, including hydrogen gas.