The enthalpy change for the reaction,

$C_{2} H_{4} (g) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 2 H_{2} O (g)$ is called:

Enthalpy of formation

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Enthalpy of combustion

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Enthalpy of vaporization

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Enthalpy of sublimation

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Solution

The correct option is B
Enthalpy of combustion

By definition, Enthalpy of combustion is the amount of heat evolved or absorbed when 1 mole of the substance is completely oxidized.

Therefore it is enthalpy of combustion

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Similar questions

Q. The enthalpy change for the following reaction, is called:

C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 {C O}_{2} (g) + 2 H_{2} O (g)

Q. The enthalpy change for the reaction,

C_{2} H_{4} (g) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 2 H_{2} O (g)

is called:

For the reaction $C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l)$ , the difference between enthalpy change and internal energy change is:

Q. The enthalpy change for the reaction,

(g) C_{2} H_{4} + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 2 H_{2} O (g)

is called:

Calculate the standard internal energy change for the reaction at 25⁰C:-

C₂H₄(g) + 3O₂(g)----------à 2CO₂ (g) + 2H₂O (l) DH for C₂H₄ (g) = 52.30 kJ/mole,

CO₂ = - 393.5 kJ/mole H₂O = - 286 kJ/mole R = 8.314 J/K/mole.

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The enthalpy change for the reaction, C2H4(g) + 3O2(g) ⟶2CO2(g) + 2H2O(g) is called:

The correct option is B Enthalpy of combustion By definition, Enthalpy of combustion is the amount of heat evolved or absorbed when 1 mole of the substance is completely oxidized. Therefore it is enthalpy of combustion

The enthalpy change for the reaction,

$C_{2} H_{4} (g) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 2 H_{2} O (g)$ is called:

The correct option is B
Enthalpy of combustion

By definition, Enthalpy of combustion is the amount of heat evolved or absorbed when 1 mole of the substance is completely oxidized.

Therefore it is enthalpy of combustion