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ForthereactionbetweenA andBA+Btoproductthefollowingratedatawereobtained . the reactionis

For the reaction below, The structure of the product 'Q' is:

For the reaction below. the structure of the product Q is

For the reaction Aunderset(k_(2)"sec"^(-1))overset(K_(1)"sec"^(-1))hArr B following graph is given, k_(1) =4 xx 10^(-@)"sec"^(-1). Which is/are correct statement (s) (In 2=0.7 , In 8/7 =0.14)

Forthe reactionbelow , (##MOD_SPJ_CHE_XII_P2_C12_E07_083_Q01.png" width="80%"> The structureof theporduct Q is

For the reaction AtoB,DeltaH=+23kJ//mol and BtoC,DeltaH=-18kJ//mol, the decreasing order of enthalpy of A,B,C follows the order

For the reaction at 500 K NO_(2)(g)+CO(g) to CO_(2)(g)+NO(g) The proposed mechanism is as follows: (i) NO_(2)+NO_(2) to NO+NO_(3) (slow) (ii) NO_(3)+CO to CO_(2)+NO_(2) (fast) What is the rate law for the reaction?

For the reaction Ato products the following dats is given for a particular run time (in): 0""5""15""35 1/([A])(M^(-1)): 1""2""4""8 Determine the order of the reaction.

For the reaction, Ato products the rate of reaction is 7.5xx10^(-4)" mole. lit"^(-1)"sec"^(-1). If the concentration of A is 0.5" mole lit"^(-1), the rate constant is

For the reaction at 500 K, "NO"_(2)(g)+"CO"(g)to"CO"_(2)(g)+"NO"(g), the proposed mechanism is as below : (i) "NO"_(2)+"NO"_(2)to"NO"+"NO"_(3)("slow")"""(ii) ""NO"_(3)+"CO"to"CO"_(2)+"NO"_(2)("fast") What is the rate law for the reaction ?

For the reaction AtoB , the rate law expression is : Rate = k[A]. Which of the following statements is incorrect?

For the reaction at 800KN_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)the ratio of K_(p)and K_(c ) is:(R = 0.082 L atm mol^(-1)K^(-1))

For the reaction at 298K, A_((g))+B_((g))rarrC_((g)) DeltaE=-5 cal and DeltaS =-10cal K^(-1)

For the reaction at 298 K : CO(g) + (1)/(2) O_(2)(g) rarr CO_(2)(g), Delta H^(@) = -282.8 kJ Standard entropies (in JK^(-1) mol^(-1)) : CO_(2)(g) = 213.6 CO(g) = 197.6 and O_(2)(g) = 205.0 Delta_(r) G^(@) for the reaction (kJ mol^(-1))

For the reaction at 25^(@)C NH_(3)(g) to (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g),DeltaH^(0)=11.04 kcal Calculate Deltau^(0) of the reaction at the given temperature.

For the reaction at 298K, Ag^+(aq)+e^-=Ag(s),E^@=+0.80VSn^(2+)(aq) +2e^- =Sn(s),E^@=-0.14V what is the emf of the cell reprsented as Sn|Sn^(2+)||Ag^+| Ag,if each ion having unit concentration:

For the reaction Ararr2B , the rate of the reaction rate is .........

For the reaction ArarrB+C, DeltaH = +25 kJ mole The activation energy for the reaction is

For the reaction A--->B,the rate law is, rate=K[A].Which of the following statement is incorrect ?

For the reaction [Ag(CN)_2]iffAg^(+) + 2CN^(-), the equilibrium constant at 25^@Cis4 xx 10^(-19) .Calculate the silver ion concentration in a solution which was originally 0.1 molar in KCN and 0.03 molar in AgNO_3 .

For the reaction: [Ag(CN)_2]^- hArrAg^+ + 2CN^- the equilibrium constant K_c at 25^@C is 4.0 xx 10^(-19) then the silver ion concentration in a solution which was originally 0.1 molar in KCN and 0.03 molar inAgNO_3

For the reaction, Ag_2O(s)to2Ag(s)+1/2O_2(g),/_\H,/_\S and T are 40kJ, 100J and 380K respectively Hence /_\Gin KJ is :

For the reaction : A(g) rarr B(g) + C(g) Concentration of 'A' varies with time (in sec) as : [A]_(T)=[10=0.2T^(2)]M The time at which rate of formation of 'B' is 1 M/sec.

For the reaction A(g) to 2B(g) (d[B])/(dt) = 6xx10^(-4) M sec^(-1) "when" [A] = 0.1 M (d[B])/(dt) = 2.4xx10^(-3) M sec^(-1) when [A] =0.4 M Find the time taken (in seconds) for concentration of A to change from 0.6 M to 0.15 M.

For the reaction A_((g)) + B_((g))hArr C_((g)) + D_((g)), the degree of dissociation alpha would be –

For the reaction A(g)+2B(g)rarr2C(g)+3D(g),the value of DeltaE at 27^(@)C is 19.0 kcal. The value of DeltaH for the reaction would be (R=2.0 cal K^(-1) mol^(-1))

For the reaction, A(g)+2B(g) to C(g)+D(g) (dx)/(dt)=k[A][B]^(2) Initial pressure of A and B are respectively 0.60 atm and 0.80 atm. At a time when pressure of C is 0.20 atm, rate of the reaction, relative to the initial value is

For the reaction AB_((g))hArrA_((g))+B_((g)), Ab is 33% dossociated at a total pressure of P. Therefore, P is related to K_(P) by one of the following options

For the reaction aC(s) + CO_2(g) hArr 2CO(g), the partial pressure of CO_2 and CO are 2.0 and4.0 atm respectively at equilibrium. TheK_p for reaction is:

For the reaction, AB(g)hArr A(g)+B(g), AB" is "33% dissociated at a total pressure of 'p' Therefore, 'p' is related to K_(p) by one of the following options

For the reaction AB_(2)(g) rarr AB(g) + B(g), the initial pressure of AB_(2)(g)was 6 atm and at equilibrium, total pressure was found to be 8 atm at 300 K. The equilibrium constant of the reaction at 300 K is……

For the reaction :A(aq) to 2B(aq) +C(aq), the rate is 2.4xx10^(-3)"mol"L^(-1)s^(-1) on 20% reaction of A and the rate is 9.6xx10^(-5)"mol" L^(-1)s^(-1) on 84% reaction of A the order of reaction is :

For the reaction : aA+bB to Product (dx)/(dt)=k[A]^(a)[B]^(b) If concentration of A is doubled, rate becomes four times. If concentration of B is made four times, rate becomes doubled . Hence

For the reactionA to B. The rate of reaction becomes three times when the concentration of A is increased by nine times. What is the order of the reaction?

For the reaction AtoB, the rate law expression is : rate = K[A]. Which of the following statements is incorrect ?

For the reaction , A to B , k_1=10^8 e^(-6000/"8.34 T") and P to Q , k_2=10^10 e^(-8000/"8.34T") The temperature at which k_1=k_2 is

For the reaction A to B, following curves represent reaction The correct curves are

For the reaction : A rarrProduct, the order of reaction is equal to :

For the reaction A rarr C, it is found that the rate of the reaction quadruples when the concentration of A is doubled. The rate for the reaction is Rate = [A]^(n). The value of n is _________

For the reaction , A overset(k)(to)B+C Following data are obtained What will be the rate of reaction (in mol L^(-1) min^(-1), when conc of 'A' is 3M.

For the reaction, A hArr B ,deltaH for the reaction is -33.0 kJ/mol. Calculate (i) Equilibrium constant K_c for the reaction at 300 K (ii) If E_a (f) and E_a(r ) in the ratio 20:31 , calculate E_a(f) at 300 K . Assuming pre-exponential factor same for forward and reverse reaction.

For the reaction A overset(K_(1))underset(K_(2))(hArr)B, if 'a' is the initial concentration of A and n is the number of moles of A reacting if initially no B was present then :

For the reaction , A hArrB : K_c =2,B hArrC : K_c =4,C hArrD : K_c =6 K_c for the reaction A hArr D is :

For the reaction A+Bto Products, the following initial rates were obtained at various given initial concentrations. ltrbgt Write rate law and find the rate constant for the above reaction.

For the reaction A+Bto products, it is found that order of A is 1 and order of B is 1//2. When concentrations of both A and B are increased four times the rate will increase by a factor

For the reaction A+Bto product ,the rate law is given by ,r=k[A]^((1)/(2))[B]^(2).What is the order of the reaction ?

For the reaction, A+Brarr"product" If concentration of A is doubled, rate increases 4 times. If concentrations of A and B both are doubled, rate increases 8 times . The differential rate equation of the reaction will be

For the reaction a+brArrc+d, initially concentrations of a and b are equal and at equilibrium the concentration of a . What will be the equilibrium constant for the reaction ?

For the reaction ,A+BrarrC+D. The variation of the concentration of the products is given by the curve: