Enthalpy of chemical adsorption- - H in kJ mol-1 is in the range of-

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Chemisorption

Enthalpy of c...

Question

Enthalpy of chemical adsorption, $Δ H$ in $k J m o l^{- 1}$ is in the range of:

500 - 1000

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40 - 400

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410 - 500

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20 - 30

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C_{2} H_{2} (g) \to C_{2} H_{4} (g) : Δ H^{\circ} = - 175 {kJ mol}^{- 1}

Δ H_{f (C_{2} H_{4}, g)}^{\circ} = 50 kJ mo l^{- 1}; Δ H_{f (H_{2} O, l)}^{\circ} = - 280 {kJ mol}^{- 1}; Δ H_{f (C O_{2} g)}^{\circ} = - 390 {kJ mol}^{- 1}

Δ H^{\circ}

{kJ mole}^{- 1}

C_{2} H_{2} (g)

∣ ∣ ∣ \frac{Δ H^{\circ}}{257} ∣ ∣ ∣

Which statements are correct ?

i) physical adsorption is due to Vander Waal’s forces

ii) physical adsorption decreases at high temperature

iii) physical adsorption is irreversible

iv) enthalpy for a chemical adsorption is generally lesser than that of physical adsorption

Δ H

k J m o l^{- 1}

Which statement is/are correct?

i) Physical adsorption is due to Vander Waal's forces

ii) Physical adsorption decreases at high temperature

iii) Physical adsorption is irreversible

iv) Enthalpy for a chemical adsorption is generally lesser than that of physical adsorption

Which statement is/are correct?

i) Physical adsorption is due to Vander Waal's forces

ii) Physical adsorption decreases at high temperature

iii) Physical adsorption is irreversible

iv) Enthalpy for a chemical adsorption is generally lesser than that of physical adsorption

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