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Polyhalogen Compounds

39. The react...

Question

39. The reaction CH3COOH(l) + C2H5OH(l) CH3COOC2H5(l) + H2O(l) was carried out at 300 K by taking 1 mol each of reactants. The reaction reached equilibrium when of reactants were consumed. Calculate Gibb’s energy change for the reaction.

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Δ G = Δ G^{\circ} + R T l n Q_{P}

Δ G = 0 and Q_{p} = K_{P}

Δ G^{\circ} = - R T l n K_{P}

K represents K_{P}

1 M or 1 atm

Δ G^{\circ} = - v e or K > 1 : forward reaction is feasible

Δ G^{\circ} = + v e or K < 1 : reverse reaction is feasible

Δ G^{\circ} = 0 or K = 1 : reaction is at equilibrium (very rare)

K_{c}

N_{2} O_{4} ⇌ 2 N O_{2}

291 K

1.14

0.5 {mol dm}^{- 3}

R = 0.082 {lit atm K}^{- 1} {mol}^{- 1}

Δ U

1742.7 k J / m o l

N H_{2} C N (s)

{N H}_{2} C N (s) + \frac{3}{2} O_{2} (g) ⟶ N_{2} (g) + {C O}_{2} (g) + H_{2} O (l)

{Δ H}_{3000 K}

(R = 8 J / m o l e - K)

\to B a S O_{4} (a q) + H_{2} O (l)

N H_{2} C N (s)

△ U

- 742.7 k J m o l^{- 1}

N H_{2} C N (g) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + C O_{2} (g) + H_{2} O (l)

N H_{2} C N (s)

Δ U

- 742.7 k J {m o l}^{- 1}

N H_{2} C N (g) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + {C O}_{2} (g) + H_{2} O (l)

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