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In an experiment starting with 1 mole of...

In an experiment starting with 1 mole of ethyl alcohol, 1 mole of acetic acid and 1 mole of water at `100^(@)C`, the equilibrium mixture on analysis shows that 54.3% of the acid is esterified. Calculate the equilibrium constant of this reaction.

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Knowledge Check

  • solution contains 1 mole of alcohol and 4 moles of water. The möle fraction of water and alcohol will be

    A
    1/4 and 7/4
    B
    4 and 1/5
    C
    1/5 and 8/5
    D
    4/5 and1/5

  • The heat of reaction at constant volme for an endothermic reaction in equilibrium is 1200 cal more than at constant pressure at 300 K. Calculate the ratio of equilibrium constant K_(p) (atm) and K_(c) (mol L^(-1) ).

    A
    `2.846 xx 10^(-3)`
    B
    `6.481 xx 10^(-3)`
    C
    `1.856 xx 10^(-3)`
    D
    `1.648 xx 10^(-3)`

  • The heat of reaction at constant volume for an endothermic reaction in equilibrium is 1200 cal more than at constant pressure at:300 K, Calculate the ratio of equilibrium constants K_(b) (atm) and K _(c) (mol L^(-1)).

    A
    `2.846 xx 10 ^(-3)`
    B
    `6.481 xx 10 ^(-3)`
    C
    `1.856 xx 10 ^(-3)`
    D
    `1.648 xx 10 ^(-3)`

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    Ethyl acetate is formed by the reaction between ethanol and acetic acid and equilibrium is represented as: 'CH_3 COOH_( )+C_2 H_5 OH_(l) hArr CH_3 COOC_2 H_5_(l)+H_2 O_(l)' i) Write the concentration ratio (reaction quotient), 'Q_c', for this reaction (note: water is not in excess and is not a solvent in this reaction) ii) At '293 K', if one starts with '1.00' mol of acetic acid and '0.18 mol' of ethanol, there is '0.171' mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant. iii) Starting with '0.5' mol of ethanol and '1.0' mol of acetic acid and maintaining it at 293 ' K, '0.214' mol of ethyl acetate is found after sometime. Has equilibrium been reached?

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