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{:(Lis - I("Reaction"), List -II((K(p))/...

`{:(Lis - I("Reaction"), List -II((K_(p))/(K_(c)))),((A)A_(2)(g) + 3B_(2)(g) hArr 2AB_(3)(g),(P)(RT)^(2)),((B) A_(2) (g)+ B_(2) (g) hArr 2 AB(g) ,(Q) (RT)^(@)),((C) A(s) + (3)/(2) B_(2) (g) hArr AB_(3)(g),(R) (RT)^(1//2)),((D) AB_(2) (g) hArr AB(g) +(1)/(2) B_(2)(g),(S) (RT)^(-1//2)):}`

Text Solution

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The correct Answer is:
A-P; B-Q; C-P; D-R
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{:(List - I , List - II),((A) N_(2) + O_(2) hArr 2NO,(p) (atm)^(-2)),((B) 2SO_(2)(g) + O_(2) hArr 2SO_(3)(g),(Q) "NO unit"),((C) H_(2) + I_(2) hArr 2HI,(R)"No cffect of pressure"),((D) N_(2)(g) + 3H_(2) (g) hArr 2NH_(3)(g), (S) "High pressure favours forward reaction"):}

{:(List - I , List - II),((A)CaCO_(3) hArr CaO + CO_(3),(P) K_(p) = K_(c)),((B) NH_(4) HS hArr NH_(3)+ H_(2)S,(Q) "High pressure favours backward reaction"),((C) PCI_(5) hArr PCI_(3) + CI_(2),(R) K_(p) = K_(c) (RT)),((D) 3Fe(s) + 4H_(2) O(g) hArr Fe_(3) O_(4) (s) + 4H_(2)(g), (S) " Heterogeneous equilibrium "):}

Knowledge Check

  • Unit of K_p for NH_4COONH_(2(s)) harr 2NH_(3(g))+ CO_(2(g)) is

    A
    No units
    B
    `atm^2`
    C
    `atm^3`
    D
    `atm^(-3)`

  • If equilibrium concentration of each component is 0.2 M , correct order of K_(C) of : I) NH_(4) HS_((s)) hArr NH_(3 (g)) + H_(2) S_((g)) II) 2 HI_((g)) hArr H_(2 (g)) + I_(2 (g)) III) PCl_(5 (g)) hArr PCl_(3 (g)) + Cl_(2 (g))

    A
    `I gt III gt II`
    B
    `I= III lt II`
    C
    `II gt III gt I`
    D
    `II gt I gt III`

  • The gascous reaction A_((g)) + B_((g)) hArr 2C_((g)) + D_((g)) + q kJ is most favoured at :

    A
    High temperature and low pressure
    B
    Low temperature and low pressure
    C
    Low temperature and high pressure
    D
    High temperature and high pressure

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    {:("Column-I (F.R.Favourable)","COlumn-II"),((A) H_(2(g)) + I_(2(g)) hArr 2HI_((g)) + Q,(P)"High temperature"),((B) 2SO_(2(g)) + O_(2(g)) hArr 2SO_(3(g)) + Q,(Q)"Low temperature "),((C) 2NH_(3(g)) hArr N_(2(g)) + 3H_(2(g)) - Q,(R)"High pressure"),((D) PCl_(5(g)) hArr PCl_(3(g)) + Cl_(2(g)) - Q,(S)"Low pressure"):}

    Derive the relation between K_(p) and K_(c) for the equilibrium reaction. N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)

    {:(Lis - I, List -II),((A)underset(("Exothermic"))( N_(2(g)) + 3H_(2(g))) hArr 2NH_(3(g)),(P)"Forward shift by rise in pressure "),((B) underset(("Exothermic"))(2SO_(2(g)) + O_(2(g))) hArr 2SO_(3(g)), (Q)"affcted by change in pressure"),((C) underset(("Endothermic"))(N_(2(g)) + O_(2(g))) hArr 2NO(g),(R)"Forward shift by rise in temperature "),((D) underset(("Endothermic"))(PCI_(5(g))) hArr PCi_(3(g))+ Cl_(2(g)),(S)"Forward shift by lowering the temperature"):}

    Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction. (i) COCl_(2)(g)hArrCO(g)+Cl_(2)(g) (ii) CH_(4)(g)+2S_(2)(g)hArrCS_(2)(g)+2H_(2)S(g) (iii) CO_(2)(g)+C(s)hArr2CO(g) (iv) 2H_(2)(g)+CO(g)hArrCH_(3)OH(g) (v)CaCO_(3)(s)hArrCaO(s)+CO_(2)(g) (vi) 4NH_(3)(g)+5O_(2)(g)hArr4NO(g)+6H_(2)O(g)

    K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2N_(3)(g) is 0.5 at 400K find K_(p)

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