Question

Methane reacts with steam at \(1273K\) in the presence of nickel catalyst to form:

• A. \(CO\) and \(H_2\)
• B. \(CO_2\) and \(H_2\)
• C. \(CO\) and \(H_2O\)
• D. \(CO_2\) and \(H_2O\)

Hint:

Steam reforming of methane gives syngas: \(\ce{CH4 + H2O → CO + 3H2}\).

Answer 1

The Correct Option is A

Step 1: Understanding the Topic:
The reaction described is known as "Steam Reforming of Methane." It is a vital industrial process covered in the chapters on "Hydrogen" and "Hydrocarbons." This method is the primary way hydrogen gas is produced globally. It involves the high-temperature catalytic reaction between a hydrocarbon and water vapor to produce a mixture of gases that serve as feedstock for further chemical synthesis.
Step 2: Key Formulas and Approach:
The approach involves identifying the specific chemical equation for the interaction between methane and water in the presence of a metal catalyst at high temperature. We analyze the oxidation state changes of carbon.
Step 3: Detailed Explanation:

Reaction Conditions: When methane ($CH_4$) and steam ($H_2O$) are passed over a Nickel ($Ni$) catalyst at approximately $1273 \text{ K}$, a redox reaction takes place.
Chemical Equation: \[ CH_4(g) + H_2O(g) \xrightarrow[1273\text{ K}]{Ni} CO(g) + 3H_2(g) \]
Products: The reaction produces Carbon Monoxide ($CO$) and Hydrogen gas ($H_2$).
Terminology: The resulting mixture of $CO$ and $H_2$ is commercially referred to as Synthesis Gas or Syngas. It is a starting point for producing methanol and other synthetic hydrocarbons. If further hydrogen is needed, the $CO$ can be reacted with more steam at a lower temperature (Water-Gas Shift reaction).
Step 4: Final Answer:
The reaction forms CO and H$_2$, corresponding to option (C).