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Carbon monoxide (CO) formation is a chemical reaction involving elements in their elemental form. In the case of CO formation, carbon (C) in solid form reacts with oxygen gas (\(\text{O}_2\)) to form carbon monoxide gas. This reaction can be represented as: \[\text{C (s)} + \frac{1}{2} \text{O}_2 (g) \rightarrow \text{CO} (g)\].

• The reaction occurs at a temperature of 298 Kelvin.
• This is an exothermic reaction, meaning it releases energy.

Understanding the molecular level of this reaction is important as carbon monoxide is a significant industrial gas and also an environmental pollutant. By comprehending its formation, we can understand its uses and how to control its emissions.

The Ideal Gas Law is a fundamental concept in chemistry that provides a simple relationship between pressure, volume, temperature, and the number of moles of a gas. It is represented by the equation: \(PV = nRT\). Here,

• \(P\) stands for pressure,
• \(V\) is volume,
• \(n\) is the number of moles of the gas,
• \(R\) is the ideal gas constant,\(8.314 \, \text{J mol}^{-1} \text{K}^{-1}\),
• \(T\) is the temperature in Kelvin.

For the reaction \(\text{C (s)} + \frac{1}{2} \text{O}_2 (g) \rightarrow \text{CO} (g)\), the Ideal Gas Law allows us to assess changes that involve gases, like the change in number of moles. Knowledge of this law helps in deriving critical calculations like \(\Delta H - \Delta U\), crucial for understanding energetics of gas-phase reactions.

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. For \(\text{C (s)} + \frac{1}{2} \text{O}_2 (g) \rightarrow \text{CO} (g)\), stoichiometry shows that one mole of carbon reacts with half a mole of oxygen gas to produce one mole of carbon monoxide gas. This calculation is key for determining the change in moles of gas \((\Delta n)\).

• Products: 1 mole of CO gas.
• Reactants: \(\frac{1}{2}\) mole of \(\text{O}_2\) gas.

The change in moles, \(\Delta n\), is calculated as: \(1 - \frac{1}{2} = \frac{1}{2}\). This value is essential in determining the energy change between enthalpy \((\Delta H)\) and internal energy \((\Delta U)\), indicating the extent of reaction under specific conditions. Stoichiometry thus forms a cornerstone of chemical calculation, linking microscopic interactions at molecular levels with observable macroscopic chemical phenomena.