Standard enthelpy of formation of carbon gas

In summary, the standard enthalpy of formation of carbon gas is 716.7 kJ, which is the energy required to form 1 mole of carbon gas from its elements in their reference form. This can be represented by the thermochemical equation C(graphite) → C(g) with a corresponding enthalpy change of 716.7 kJ. This does not mean that adding 716.7 kJ of energy will increase the temperature to 4827.0 °C, as temperature is not directly equivalent to energy.
  • #1
mcfaker
43
0
Hi,

The standard enthalpy of formation of carbon gas or C(g) is the enthalpy change for the formation of 1 mole of carbon gas from its elements in their reference form which for carbon (I believe) is C(graphite).

Now I find the following standard enthalpy of formation for carbon gas / C(g) : 716.7 kJ

So now the formation reaction(or thermochemical equatation) is:

C(graphite) → C(g) ΔH= 716.7 kJ

Am I right? So if we add 716,7kJ to 1 mole of graphite ( note: not diamond) we will get carbon gas? Now carbon gas only excists at a temperature of 4827.0 °C so that means if we add 716.7 kJ it will increase the temperature up to 4827.0 °C?


Thanks in advance!
 
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  • #2
Temperature is not the equivalent of energy.
 

FAQ: Standard enthelpy of formation of carbon gas

What is the standard enthalpy of formation of carbon gas?

The standard enthalpy of formation of carbon gas (CO2) is defined as the change in enthalpy that occurs when one mole of carbon gas is formed from its constituent elements in their standard states (solid carbon and gaseous oxygen) at a temperature of 298K and a pressure of 1 bar.

Why is the standard enthalpy of formation of carbon gas important?

The standard enthalpy of formation of carbon gas is important because it is used as a reference point for calculating the enthalpy of reactions involving carbon gas. It also provides information about the stability of carbon gas and its potential to release energy when formed.

How is the standard enthalpy of formation of carbon gas determined?

The standard enthalpy of formation of carbon gas is determined experimentally using calorimetry. In this method, the enthalpy change of a reaction involving carbon gas is measured and then compared to the known enthalpy changes of other reactions involving the same elements. The difference between the two values gives the standard enthalpy of formation of carbon gas.

What is the significance of the standard state in calculating the standard enthalpy of formation of carbon gas?

The standard state is a specific set of conditions (temperature, pressure, and physical state) that is used as a reference point for thermodynamic calculations. In the case of the standard enthalpy of formation of carbon gas, the standard state for carbon is solid and for oxygen is gas. This ensures that the enthalpy of formation is measured under consistent conditions for accurate comparisons.

How does the standard enthalpy of formation of carbon gas differ from the standard enthalpy of combustion of carbon gas?

The standard enthalpy of formation of carbon gas is the enthalpy change when carbon gas is formed from its constituent elements, whereas the standard enthalpy of combustion is the enthalpy change when one mole of carbon gas undergoes complete combustion to form carbon dioxide gas. The standard enthalpy of combustion of carbon gas is typically a larger negative value compared to the standard enthalpy of formation, as the combustion process releases more energy.

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