At constant T and P- which one of the following statements is correct for the reaction- CO g -1-2 O 2 g - CO 2 g A- - H is independent of the physical state of the reactants of that compound B- - H - EC- - H - ED- - H - E

The correct option is C Δ H lt; Δ EΔ n_g=1 3/2= 1/2, As Δ n_g is negative, thus Δ H lt; Δ E ...

Difference between Internal Energy and Enthalpy

At constant T...

Question

At constant T and P, which one of the following statements is correct for the reaction, $C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)$

Δ H

is independent of the physical state of the reactants of that compound

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Δ H > Δ E

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Δ H < Δ E

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Δ H = Δ E

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C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)

Which of the following statements is correct for the reaction $C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)$ at constant temperature and pressure?

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)

C_{6} H_{10}

C O (g)

C O_{2} (g)

Δ H = - 110

Δ H = - 393 k J m m o l^{- 1}

(Δ H)

m o l^{- 1}

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)

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