For a reversible reaction aA + bBhArrcC ...

For a reversible reaction `aA + bBhArrcC + dD` , the variation of K with temperature is given by

`K_(2) gt K_(1)` if `T_(2) gt T_(1)` for an endothermic change

`K_(2) lt K_(1)` if `T_(2) gt T_(1)` for an endothermic change

`K_(2) gt K_(1)` if `T_(2) gt T_(1)` for an exothermic change

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For a reaction, aA+bBhArrcC+dD , the reaction quotient Q=([C]_(0)^(c)[D]_(0)^(d))/([A]_(0)^(a)[B]_(0)^(b)) , where [A]_(0) , [B]_(0) , [C]_(0) , [D]_(0) are initial concentrations. Also K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)) where [A] , [B] , [C] , [D] are equilibrium concentrations. The reaction proceeds in forward direction if Q lt K_(c) and in backward direction if Q gt K_(c) . The variation of K_(c) with temperature is given by: 2303log(K_(C_(2)))/(K_(C_(1)))=(DeltaH)/(R)[(T_(2)-T_(1))/(T_(1)T_(2))] . For gaseous phase reactions K_(p)=K_(c)(RT)^(Deltan) where Deltan= moles of gaseous products - moles of gaseous reactants. Also -DeltaG^(@)=2.303RT log_(10)K_(c) . The heat or reaction for an endothermic reaction, in equilibrium is 1200 cal , at constant volume is more than at constant pressure at 300 K . The ratio of K_(p)//K_(c) is:

For a reaction, aA+bBhArrcC+dD , the reaction quotient Q=([C]_(0)^(c)[D]_(0)^(d))/([A]_(0)^(a)[B]_(0)^(b)) , where [A]_(0) , [B]_(0) , [C]_(0) , [D]_(0) are initial concentrations. Also K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)) where [A] , [B] , [C] , [D] are equilibrium concentrations. The reaction proceeds in forward direction if Q lt K_(c) and in backward direction if Q gt K_(c) . The variation of K_(c) with temperature is given by: 2303log(K_(C_(2)))/(K_(C_(1)))=(DeltaH)/(R)[(T_(2)-T_(1))/(T_(1)T_(2))] . For gaseous phase reactions K_(p)=K_(c)(RT)^(Deltan) where Deltan= moles of gaseous products - moles of gaseous reactants. Also -DeltaG^(@)=2.303RT log_(10)K_(c) . The equilibrium constants for the reaction, CaC_(2(s))+5O_(2(g))hArr2CaCO_(3(s))+2CO_(2(g)) is//are given by:

For a reaction, aA+bBhArrcC+dD , the reaction quotient Q=([C]_(0)^(c)[D]_(0)^(d))/([A]_(0)^(a)[B]_(0)^(b)) , where [A]_(0) , [B]_(0) , [C]_(0) , [D]_(0) are initial concentrations. Also K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)) where [A] , [B] , [C] , [D] are equilibrium concentrations. The reaction proceeds in forward direction if Q lt K_(c) and in backward direction if Q gt K_(c) . The variation of K_(c) with temperature is given by: 2303log(K_(C_(2)))/(K_(C_(1)))=(DeltaH)/(R)[(T_(2)-T_(1))/(T_(1)T_(2))] . For gaseous phase reactions K_(p)=K_(c)(RT)^(Deltan) where Deltan= moles of gaseous products - moles of gaseous reactants. Also -DeltaG^(@)=2.303RT log_(10)K_(c) . ( B ) The moisture content of a gas is often expressed as dew point, the temperature at which if gas is cooled becomes saturted with vapour pressure of water at that temperture. Dew point of H_(2)O is 43^(@)C having vapour pressure 0.07 "torr" . CaCl_(2)*2H_(2)O_((s))hArrCaCl_(2(s))+2H_(2)O_((g)) , The equilibrium constant should not be more than..... (atm)^(2) if CaCl_(2) is to be used as desiccant.

For a reaction, aA+bBhArrcC+dD , the reaction quotient Q=([C]_(0)^(c)[D]_(0)^(d))/([A]_(0)^(a)[B]_(0)^(b)) , where [A]_(0) , [B]_(0) , [C]_(0) , [D]_(0) are initial concentrations. Also K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)) where [A] , [B] , [C] , [D] are equilibrium concentrations. The reaction proceeds in forward direction if Q lt K_(c) and in backward direction if Q gt K_(c) . The variation of K_(c) with temperature is given by: 2303log(K_(C_(2)))/(K_(C_(1)))=(DeltaH)/(R)[(T_(2)-T_(1))/(T_(1)T_(2))] . For gaseous phase reactions K_(p)=K_(c)(RT)^(Deltan) where Deltan= moles of gaseous products - moles of gaseous reactants. Also -DeltaG^(@)=2.303RT log_(10)K_(c) . ( A ) A hydrated salt show efflorescent nature by lossing water molecule . Under what pressure of moisture in atmosphere, CuSO_(4)*5H_(2)O will show efflorescence bature if CuSO_(4)*5H_(2)O_((s))hArrCuSO_(4)*3H_(2)O+2H_(2)O_((v)) , K_(p)=62.72 mm^(2) ?

For a reaction, aA+bBhArrcC+dD , the reaction quotient Q=([C]_(0)^(c)[D]_(0)^(d))/([A]_(0)^(a)[B]_(0)^(b)) , where [A]_(0) , [B]_(0) , [C]_(0) , [D]_(0) are initial concentrations. Also K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)) where [A] , [B] , [C] , [D] are equilibrium concentrations. The reaction proceeds in forward direction if Q lt K_(c) and in backward direction if Q gt K_(c) . The variation of K_(c) with temperature is given by: 2303log(K_(C_(2)))/(K_(C_(1)))=(DeltaH)/(R)[(T_(2)-T_(1))/(T_(1)T_(2))] . For gaseous phase reactions K_(p)=K_(c)(RT)^(Deltan) where Deltan= moles of gaseous products - moles of gaseous reactants. Also -DeltaG^(@)=2.303RT log_(10)K_(c) . The equilibrium constant K_(c) for A_((g))hArrB_((g)) is 1.1 . The gas having concentration ge 1 is:

For a certain reaction the variation of rate constant with temperature is given by the equation ln k_(t) = lnk_(0) + ((ln 3)t)/(10) (t ge 0^(@)C) The value of temperature coefficient of the reaction is

For an elementary reaction the variation of rate constant (k) with temperature is given by the following equation log_(10) k=5.4 -100/T Where, T is temperature on Kelvin scal and k is in terms of sec^(-1) Identify the incorrect options.

MOTION-CHEMICAL EQUILIBRIUM-Exercise - 2

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