When 1 mole co gas is produced from its elements in standard state at 298k temprature, then what will be the value of deltaH -deltaE?

To determine the value of ΔH - ΔE when 1 mole of carbon monoxide (CO) gas is produced from its elements in their standard states at 298 K, we need to understand the relationship between enthalpy (ΔH) and internal energy (ΔE). This relationship is expressed by the equation:

Understanding the Relationship

The equation connecting enthalpy and internal energy is:

ΔH = ΔE + ΔnRT

In this equation:

• ΔH is the change in enthalpy.
• ΔE is the change in internal energy.
• Δn is the change in the number of moles of gas during the reaction.
• R is the universal gas constant (approximately 8.314 J/(mol·K)).
• T is the temperature in Kelvin.

Calculating Δn

For the formation of carbon monoxide from its elements, the balanced chemical equation is:

C(s) + 1/2 O2(g) → CO(g)

In this reaction, we start with 1 mole of solid carbon and 0.5 moles of oxygen gas, resulting in 1 mole of carbon monoxide gas. Thus, the change in the number of moles of gas (Δn) is:

Δn = moles of products - moles of reactants = 1 - 0.5 = 0.5

Substituting Values

Now we can substitute Δn into the equation:

ΔH = ΔE + (0.5)(8.314 J/(mol·K))(298 K)

Calculating the term:

ΔH = ΔE + 0.5 × 8.314 × 298

ΔH = ΔE + 1239.57 J

Finding ΔH - ΔE

To find ΔH - ΔE, we can rearrange the equation:

ΔH - ΔE = 1239.57 J

Final Result

Therefore, when 1 mole of carbon monoxide gas is produced from its elements in standard state at 298 K, the value of ΔH - ΔE is approximately:

ΔH - ΔE = 1239.57 J

This result illustrates how the energy changes during the formation of a gas from its elemental states, highlighting the importance of understanding thermodynamic principles in chemical reactions.