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| 29451. |
The integrated rate equations isRtt="log"C_(0)-"log"C_(r) The straight line graph is obtained by plotting |
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Answer» timesVs`"log"C_(t)` |
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| 29452. |
The integrated rate equation is Rt = log C_(0)- logC_(t). The straight line graph is obtained by plotting |
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Answer» TIME v/s log `C_(t)` |
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| 29453. |
The integrated rate equation for first order reaction A rarr productsis given by |
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Answer» `K=(2.303)/(t)ln.([A]_(0))/([A]_(t))` |
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| 29454. |
The instrument which can be used to measure optical activity, i.e., specific rotation: |
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Answer» Refractometer |
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| 29455. |
The integrated rate equation for first order reaction is A to products. |
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Answer» K=2.303 t `log_(10) ([A]_(0))/([A]_(t))` |
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| 29456. |
theintegrated rateequationforfirstorderreaction A toproducts is given by |
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Answer» `L=(2.303)/(t)l n ([A_(0)])/([A_(t)])` |
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| 29457. |
The instantaneous rate of an elementary chemical reaction aA+bB (hArr)cC+dD can be given by: rate =k_(f)[A]^(a)[B]^(b)-k_(b)[C]^(c)[D]^(d) where k_(f) and k_(b) are rate constants for forward and backward reactions respectively for the reversible reaction if the reaction is an irreversible one , the rate is expressed as rate =k[A]^(a)[B]^(b) where k is rate constant for the given irreversible reaction and (a+b) is the order of reaction it is also evident from the stoichiometry of reaction that rates of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant k with temperature is expressed in terms of Arrhenius equation:k=Ae^-(E_(a)//RT) whereas the ratio k_(f)/k_(b) is expressed in terms of van't Hoff isochore: K_(f)/K_(b)=Ae^(-DeltaH//RT) where E_(a) and DeltaH are energy of activation and enthalpy of reaction respectively For an elementary reaction aA rarrproduct the graph plotted between log [-(d[A])/(dt)] vs. concentration gives a straight line with intercept equal to 0.6 and showing an angle of 45^(@) with origin, then: |
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Answer» RATE constant `=3.98 time^(-1) and a=1` |
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| 29458. |
The instrument in which combustion energy of fuel like hydrogen and methane is directly converted to electrical energy is known as. . . |
| Answer» Solution :Fuel cell. | |
| 29459. |
The instantaneous rate of an elementary chemical reaction aA+bB (hArr)cC+dD can be given by: rate =k_(f)[A]^(a)[B]^(b)-k_(b)[C]^(c)[D]^(d) where k_(f) and k_(b) are rate constants for forward and backward reactions respectively for the reversible reaction if the reaction is an irreversible one , the rate is expressed as rate =k[A]^(a)[B]^(b) where k is rate constant for the given irreversible reaction and (a+b) is the order of reaction it is also evident from the stoichiometry of reaction that rates of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant k with temperature is expressed in terms of Arrhenius equation:k=Ae^-(E_(a)//RT) whereas the ratio k_(f)/k_(b) is expressed in terms of van't Hoff isochore: K_(f)/K_(b)=Ae^(-DeltaH//RT) where E_(a) and DeltaH are energy of activation and enthalpy of reaction respectively For a gaseous phase Ist order reaction A(g) rarr B(g)+2C(g) (rate constant K=10^(-2)time^(-1)) in a closed vessel of 2 litre containing 5 mole of A(g) at 27^(@) C which of the following is incorrect? |
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Answer» Rate of a appearance of `C(g) is 5XX10^(-2) MOL L^(-1)t^(-1)` |
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| 29460. |
The instantaneous rate of an elementary chemical reaction aA+bB (hArr)cC+dD can be given by: rate =k_(f)[A]^(a)[B]^(b)-k_(b)[C]^(c)[D]^(d) where k_(f) and k_(b) are rate constants for forward and backward reactions respectively for the reversible reaction if the reaction is an irreversible one , the rate is expressed as rate =k[A]^(a)[B]^(b) where k is rate constant for the given irreversible reaction and (a+b) is the order of reaction it is also evident from the stoichiometry of reaction that rates of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant k with temperature is expressed in terms of Arrhenius equation:k=Ae^-(E_(a)//RT) whereas the ratio k_(f)/k_(b) is expressed in terms of van't Hoff isochore: K_(f)/K_(b)=Ae^(-DeltaH//RT) where E_(a) and DeltaH are energy of activation and enthalpy of reaction respectively The variation of K and K_(f)/K_(b) with increase in temperature shows the following effects: (P) For endothermic reaction K increases, K_(f)/K_(b) also increases (Q) For exothermic reaction K decreases K_(f)/K_(b) also decreases (R) For exothermic reaction K and K_(f)/K_(b) both increases (S) For exothermic reaction K increases and K_(f)/K_(b) decreases (T) For exothermic reaction K and K_(f)/K_(b) both decreases. |
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Answer» <P>(P),(S) |
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| 29461. |
The instantaneous rate of an elementary chemical reaction aA+bB (hArr)cC+dD can be given by: rate =k_(f)[A]^(a)[B]^(b)-k_(b)[C]^(c)[D]^(d) where k_(f) and k_(b) are rate constants for forward and backward reactions respectively for the reversible reaction if the reaction is an irreversible one , the rate is expressed as rate =k[A]^(a)[B]^(b) where k is rate constant for the given irreversible reaction and (a+b) is the order of reaction it is also evident from the stoichiometry of reaction that rates of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant k with temperature is expressed in terms of Arrhenius equation:k=Ae^-(E_(a)//RT) whereas the ratio k_(f)/k_(b) is expressed in terms of van't Hoff isochore: K_(f)/K_(b)=Ae^(-DeltaH//RT) where E_(a) and DeltaH are energy of activation and enthalpy of reaction respectively For a chemical reaction :aA rarr bB log[(d[A])/(dt)]=log [(d[B])/(dt)+0.3 Then the ratio of a and b is approximately: |
| Answer» ANSWER :C | |
| 29462. |
The instantaneous rate of an elementary chamical reactkon aA+bBhArr cC+dD can be given by rate =K_(f)[A]^(a)[B]^(b)-K_(b)[C]^(c)[D]^(d) where K_(f) and K_(b) are rate constants for forward and backward reactions respectively for the reversiblereaction. If the reaction is an irreversible one, the rate is expressed as, rate =K[A]^(a)[B]^(b) where K is rate contant for the given irreversible rate of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant K with temperature is expressed in terms of Arrheniusequation: K=Ae^(-E_(a)//RT) whereasthe ratio (K_(f))/(K_(b)) is expressed in terms of van't Hoff isochore: (K_(f))/(K_(b))=Ae^(-DeltaH//RT), where E_(a) and DeltaH are energy of activation and heat of reaction respectively. For an elementary reaction aAto product, the graph plotted log([-d[A]])/(dt) vs log[A]_(t) gives a straight line with intercept equal to 0.6 and showing an angle of 45^(@) then |
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Answer» rate constant =4`"time"^(-1)` and a=1 Here `a=1,logK=log4,K=4` |
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| 29463. |
The instantaneous rate of an elementary chamical reactkon aA+bBhArr cC+dD can be given by rate =K_(f)[A]^(a)[B]^(b)-K_(b)[C]^(c)[D]^(d) where K_(f) and K_(b) are rate constants for forward and backward reactions respectively for the reversiblereaction. If the reaction is an irreversible one, the rate is expressed as, rate =K[A]^(a)[B]^(b) where K is rate contant for the given irreversible rate of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant K with temperature is expressed in terms of Arrheniusequation: K=Ae^(-E_(a)//RT) whereasthe ratio (K_(f))/(K_(b)) is expressed in terms of van't Hoff isochore: (K_(f))/(K_(b))=Ae^(-DeltaH//RT), where E_(a) and DeltaH are energy of activation and heat of reaction respectively. For a gaseous phase -I order reaction A(g)toB(g)+2C(g) (rate constant K=10^(-2)"time"^(-1)) in a closedvesel of 2 litre containing 5 mole of A(g) at 27^(@)C which of the following is correct? |
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Answer» Rate of appearance of C (g) is `5xx10^(-2),"mol"L^(-1)t^(-1)` |
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| 29464. |
The instantaneous rate of an elementary chamical reactkon aA+bBhArr cC+dD can be given by rate =K_(f)[A]^(a)[B]^(b)-K_(b)[C]^(c)[D]^(d) where K_(f) and K_(b) are rate constants for forward and backward reactions respectively for the reversiblereaction. If the reaction is an irreversible one, the rate is expressed as, rate =K[A]^(a)[B]^(b) where K is rate contant for the given irreversible rate of disappearance of A is a/b times the rate of disappearance of B. The variation of rate constant K with temperature is expressed in terms of Arrheniusequation: K=Ae^(-E_(a)//RT) whereasthe ratio (K_(f))/(K_(b)) is expressed in terms of van't Hoff isochore: (K_(f))/(K_(b))=Ae^(-DeltaH//RT), where E_(a) and DeltaH are energy of activation and heat of reaction respectively. The variation of rate constant K and (K_(f))/(K_(b)) with temperature shows the following effects: For endothrmic reaction when T increases then K increases and (K_(f))/(K_(b)) also increases. (ii) For endothemic reaction when T decreases then K decreases and (K_(f))/(K_(b)) also decreases. (iii) For exothermic when T increases then K and (K_(f))/(K_(b)) both increases. (iv) For exothermic reaction when T decreases then K increases and (K_(f))/(K_(b)) decrease. (v) For exothermic reaction when T increases thenK and (K_(f))/(K_(b)) both decrease. |
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Answer» I,ii |
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| 29465. |
The insecticidegermicide gammexane is a formulation for : |
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Answer» DDT |
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| 29466. |
The insecticide containing 99% of 7 isomer of Benzene hexachloride is known as |
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Answer» PDT |
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| 29467. |
The insecticide, germicide, gammesane is a formulation for: |
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Answer» `DDT` |
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| 29468. |
The inreasing order of O-N-O bond angel in the species NO_(2), NO_(2)^(+) and NO_(2)^(-) is |
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Answer» `NO_(2)^(+) LT NO_(2) lt NO_(2)^(-)` |
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| 29469. |
The inorganic compound that on heating gives organic compound is |
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Answer» Sodamide |
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| 29470. |
The insecticide containing 99% gamma-isomer of benzene hexachloride is known as : |
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Answer» Lindane |
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| 29471. |
The inorganic origin of petroleum is indicated by the fact that |
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Answer» It CONSTITUENTS can be separated by FRACTIONAL distillation |
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| 29472. |
The inorganic cation in the question above could be |
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Answer» nickel `Al(OH)_3 + 3H^(+)to Al^( + ++) + 3H_2O` `Al(OH)_3 + OH^(-) to Al(OH)_4` |
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| 29473. |
The inorganic benzene is name given to to : |
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Answer» `B_(3)N_(3)H_(6)` |
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| 29474. |
The inner transition elements are the elements in which the added electrons go to : |
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Answer» (n-1) d-ORBITALS |
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| 29475. |
The inner orbital complex which exhibits both geometrical as well as optical isomerism. |
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Answer» `[Cr(en)_(3)]^(3+)` |
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| 29476. |
The inner lining of a blast furnace is made up of |
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Answer» GRAPHITE bricks |
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| 29477. |
The initial rates ofreaction 3A + 2B + C to Products, at different initial concentrations are given below: The order with respect to the reactants, A, B and Care respectively |
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Answer» 3, 2, 0 From `1^(st)` and `4^(th)` sets of data Dividing EQ. (4) by eq. (1) `(1.25 xx 10^(-3))/(5.0 xx 10^(-3))=[(0.005)/(0.010)]^(X)` or `0.25=(0.5)^(x)` or `(0.5)^(2)=(0.5)^(x)` `:. x = 2` The order with respect to .A. is 2 from the `1^(st)` and `3^(rd)` sets of data Dividing eq. (1) by eq. (3) `(5.0 xx 10^(-3))/(1.0 xx 10^(-2))=[(0.005)/(0.010)]^(y)` or `(0.5)^(1)=(0.5)^(y)implies y = 1` The order with respect to .B. is 1 So the order with respective the reactants A, B and C is 2, 1 and 0. |
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| 29478. |
The initial ratio of hydrolysis of methyl acetate (1 M) by a weak acid (HA, 1M) is 1//100^(th) of that of a strong acid (HX, 1M) at 25^(@)C. The K_(a) of HA is |
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Answer» `1 xx 10^(-4)` `(R_(HA))/(R_(HA)) = ([H^(+)]_(HA))/([H^(+)]_(HX))` `(1)/(100) = [H^(+)]_(HA)` `{:(HA,H^(+),+,A^(-)),(1-0.01,0.01,0.01,),(~~1,,,):}` `K_(a) = (0.01 xx 0.01)/(1) = 10^(-4)` |
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| 29479. |
The initial rates of reaction 3A + 2B + C to Products, at different initial concentrations are given below The order with the respect to the reactants A, B and C are respectively. |
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Answer» 3,2,0 Rate =`k[A]^(p)[B]^(Q)[C]^( r)` By compairing the data from 1st and 2nd sets, the concentration of 'A' and 'B' are constants. When the concentration of 'C' is made thrice, there is no change in the initial rate. `therefore` The order with respect to `c'`=0 Now, let us compare data from 3RD and 1st sets. `(1.0 xx 10^(-2))/(5.0 xx 10^(-3))= (0.010)^(q)/(0.005)^(q)` `(2)^(1) = (2)^(q)` Order with respect to B=1 Now, let us compare data from 4th and 1st sets.s `(1.25 xx 10^(-3))/(5.0 xx 10^(-3)) = (0.005)^(p)/(0.010)^(p)` `(1/4) = (1/2)^(p)` `(1/2)^(2) = (1/2)^(p)` Order with respect to A=2 Thus, the order with respect to A, B and C are: 2,1,0. Thus, the order with respect to A, B and C are: 2,1,0. |
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| 29480. |
The initial rates of reaction 3" A"+2" B"+" C"to Products, at different initial concentrations are given below : {:("Initial rate, "Ms^(-1),,,[A]_(0)","M,,,[B]_(0)","M,,,[C]_(0)","M),(5.0xx10^(-3),,,0.010,,,0.005,,,0.010),(5.0xx10^(-3),,,0.010,,,0.005,,,0.015),(1.0xx10^(-2),,,0.010,,,0.010,,,0.010),(1.25xx10^(-3),,,0.005,,,0.005,,,0.010):} The order with respect to the reactants A, B and C are respectively |
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Answer» `3, 2, 0` `5*0 xx 10^(-3) = (0*010)^(alpha) (0.005)^(beta) (0.010)^(gamma)""…(i)` `5*0 xx 10^(-3) = (0*10)^(alpha)(0.005)^(beta) (0*015)^(gamma)""…(ii)` `1*0 xx 10^(-2) = (0*010)^(alpha) (0*010)^(beta) (0.010)^(gamma) ""...(iii)` `1*25 xx 10^(-3) = (0*005)^(alpha)(0.005)^(beta) (0.010)^(gamma)""...(iv)` Dividing (i) by (ii) 1=((0*010)/(0*015))^(gamma)or((2)/(3))^(gamma)=1=((2)/(3))^(0)thereforegamma=0` Dividing (iii) by (ii), `(1*0 xx 10^(-2))/(5*0 xx 10^(-3)) = (2)^(beta) ((2)/(3))^(gamma) or 2 = (2)^(beta) ((2)/(3))^(0) = 2^(beta)` or `2^(beta) = 2 or beta =1.` Dividing (i) by (iv), 4 = `(2)^(alpha) or alpha = 2 ` `therefore` Orders w.r.t. A , B and C are 2, 1, 0. |
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| 29481. |
The initial rates for gaseous reaction A+3BtoAB_(3) are given below [A](M)""[B](M)"""Rate(Msec"^(-1)) 0.1""0.1""0.002 0.2""0.1""0.002 0.3""0.2""0.008 0.4""0.3""0.018 order of reaction is |
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Answer» zero |
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| 29482. |
The initial rate of reaction A + B to C, was measured for several concentration of A and B. The decomposition made are recorded in the following table. Using the data in the above table, determine a) the rate law for the reason b) the magnitude of the rate constant. |
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Answer» Rate =`k[A]^(p)[B]^(q)` Comparing experiments (1) and (2), `("Rate")_(1)=k[0.1]^(p)[0.1]^(q)=4.0 xx 10^(-5)`…………(i) `("Rate")_(2) = k[0.1]^(p)[0.2]^(q)=4.0 xx 10^(-5)`…………….(ii) DIVIDING EQN. (ii) by (i), `("Rate")_(2)/("Rate")_(1) = (k[0.1]^(p)[0.2]^(q))/(k[0.1]^(p)[0.1]^(q))/(k[0.1]^(p)[0.1]^(q)) = (4.0 xx 10^(-5))/(4.0 xx 10^(-5))` =1 `[2]^(q) = [2]^(0)` or q=0 Comparing experiments (1) and (3), `("Rate")_(1) = (k[0.1]^(p)[0.1]^(q))/([k[0.1]^(p)[0.1]^(q))) = (16.0 xx 10^(-5))/(4.0 xx 10^(-5)) = 4=[2]^(p)=[2]^(q)` or p=2 Order w.r. to A=2, Order w.r. to B=0 Rate law for the reaction `=k[A]^(2)` VALUE of rate constant from expt:1. `(4.0 xx 10^(-5) mol L^(-1)s^(-1)) =k[A] = k(0.1 mol L^(-1))^(2)`. `k=(4.0 xx 10^(-5) mol L^(-1)s^(-1))/(0.1 mol L^(-1))^(2) = 4.0 xx 10^(-3) L mol^(-1)s^(-1)` |
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| 29483. |
The initial rate of reaction A+5B+6Cto3L+3M has been determined by measuring the rate of disappearance of A under the following conditions : {:("Expt. No.",,,[A]_(0)//M,,,[B]_(0)//M,,,[C]_(0)//M,,,"Initial rate"//"M min"^(-1)),(1,,,0.02,,,0.02,,,0.02,,,2.08xx10^(-3)),(2,,,0.01,,,0.02,,,0.02,,,1.04xx10^(-3)),(3,,,0.02,,,0.04,,,0.02,,,4.16xx10^(-3)),(4,,,0.02,,,0.02,,,0.04,,,8.32xx10^(-3)):} Determine the order of reaction with respect to each reactant and overall order of the reaction. What is the rate constant ? Calculate the initial rate of change in concentration of B and L. |
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Answer» Initial rate `=-(1)/(5)(d[B])/(dt)=+(1)/(3)(d[L])/(dt)=2.08xx10^(-3)" M min"^(-1)"(Given)"` `:." Initial change in conc. of B, i.e., "(d[B])/(dt)=-5xx(2.08xx10^(-3))=-1.04xx10^(-2)" M min"^(-1)` Initial change in conc. of L, i.e., `(d[L])/(dt)=3xx(2.08xx10^(-3))=6.24xx10^(-3)" M min"^(-1)` |
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| 29484. |
The initial rate of hydrolysis of methyl acetate (1" M") by a weak acid (HA, 1 M) is 1//100th of that of a strong acid (HX, 1 M) at 25^(@)C. The K_(a) of HA is |
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Answer» `1xx10^(-4)` Rate w.r.t. strong acid, `R_2=k[H^+]_(SA)` [ ester ] `:.""R_1/R_2=([H^+]_(WA))/([H^+]_(SA))=1/100"(Given)"` `:.""[H^+]_(WA)=([H^+]_(SA))/(100)=1/100xx1M=0.01M` `=10^(-2)M` `HAhArrH^++A^-` Initial`"C mol L"^-1` At eqm. ` C-Calpha""Calpha""Calpha` `=C(1-alpha)` `[H^+]=Calpha" or "10?^-2=1xxalpha" or "alpha=10^-2` `K_a=(Calpha.Calpha)/(C(1-alpha))=(Calpha^2)/(1-alpha)~~Calpha^2` `=1xx(10^-2)=10"^-4` |
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| 29485. |
The initial rate of a first order reaction is 5.2 xx 10^(-6)" mol.lit"^(-1).s^(-1) at 298 K. When the initial concentration of reactant is 2.6xx10^(-3)" mol.lit"^(-1), calculate the first order rate constant of the reaction at the same temperature. |
| Answer» SOLUTION :`2XX10^(-3)s^(-1)` | |
| 29486. |
The initial rate , -(d [A])/(dt) at t = 0 was found to be 2 . 6 xx 10^(-2) mol L^(-1) s^(-1)for the reaction A + 2B toProducts The initial rate , - (d[B])/(dt) at t= 0 is |
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Answer» `0.01` MOL `L^(-1) s^(-1)` `-(d[A])/(dt) = (-d[B])/(2dt)` `2.6 xx 10^(-2)` mol `L^(-1) s^(-1) = (-d[B])/(2dt)` `(-d[B])/(dt) = 2 xx 2.6 xx 10^(-2)` `= 5.2 xx 10^(-2)` mol `L^(-1) s^(-1)` |
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| 29487. |
The initial rate of a first order reaction is 5.2xx10^(-6) "mol lit"^(-1)s^(-1) 298 K. When the initial concentration of reactant is 2.6xx10^(-3)"mol lit"^(-1), calculate the first order rate constant of the reaction at the same temperature. |
| Answer» SOLUTION :`2XX10^(-3)s^(-1)` | |
| 29488. |
The initial concentrations or pressure of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the directions in which each system will shift to reach equilibrium. 2NO(g)+Cl_(2)(g)hArr2NOCl(g) K = 4.6 ×x 10^(4) [NO]=1.00 M , [Cl_(2)] = 1.00 M ,[NOCl] = 0 M |
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Answer» |
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| 29489. |
The initial concentrations or pressure of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the directions in which each system will shift to reach equilibrium. 2SO_(3)(g)hArr2SO_(2) (g) + O_(2)(g) K_(p) = 16.5 atm Initial pressure : SO_(3) = 1.0 atm, SO_(2) = 1.0 atm , O_(2) = 1.0 atm |
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Answer» |
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| 29490. |
The initial concentrations or pressure of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the directions in which each system will shift to reach equilibrium. 2NH_(3) (g)hArr N_(2)(g)+3H_(2)(g) K_(p)=6.8 x× 10^(4) atm^(2) Initial pressure : NH_(3) = 3.0 atm , N_(2) = 2.0 atm , H_(2) = 1.0 atm |
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Answer» |
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| 29491. |
The IUPAC name of C_2H_5OCH_2CH(CH_3)_2 is , |
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Answer» 3-ethoxy -2-methylpropane |
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| 29492. |
The initial concentrations or pressure of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the directions in which each system will shift to reach equilibrium. 2SO_(3)(g)hArr2SO_(2)(g)+O_(2)(g) K = 0.230 atm [SO_(3)]=0.00 M,[SO_(2)]= 1.00 M ,[O_(2)] = 1.00 M |
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Answer» |
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| 29493. |
The IUPAC name of C_(2)H_(5)-overset(CH_(2))overset(||)(C)-CH_(2)-overset(CH_(3))overset(|)(CHNH_(2) is: |
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Answer» 4-amino-2-ethylpent-1-ene |
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| 29494. |
The IUPAC name of (C_(2)H_(5))_(2)CHCH_(2)OH is : |
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Answer» 2-Ethyl butan-1-ol |
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| 29495. |
The initial concentrations or pressure of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the directions in which each system will shift to reach equilibrium. 2NH_(3) (g) hArrN_(2)(g) + 3H_(2)(g) K = 17 [NH_(3)] = 0.20 M , [N_(2)] = 1.00 M , [H_(2)]=1.00 M |
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Answer» |
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| 29496. |
The IUPAC name of C_(2)H_(5) -O-CH(CH_(3))_(2) |
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Answer» ETHOXY propane |
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| 29497. |
The initial concentrations of X and Y were 2 and 4 moles/litre respectively for the following equilibrium X+2YhArrZ. Which of the following relationships among equilibrium concentrations of X, Y and Z is (are) not feasible? |
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Answer» [X] = [Z] |
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| 29498. |
The IUPAC name of C_(2)H_(5)-O-CH_(2)-CH(CH_(3))_(2) is |
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Answer» 1-Ethoxy-1-butane |
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| 29499. |
The IUPAC name of BrCH_(2)underset(CONH_(2))underset(|)(CHCOCH_(2))CH_(2)CH_(3), is: |
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Answer» 2-bromomethyl-3-oxohexanamide |
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| 29500. |
The initial concentration of N_(2)O_(5)to 2NO_(2(g))+(1)/(2)O_(2(g)) was 1.24xx10^(-2) mol L^(-1) at 300 K temperature .The concentration of N_(2)O_(5) after 60 minutes was 0.2xx10^(-2) mol L^(-1).Calculate the rate constatn of the reaction . |
| Answer» SOLUTION :`0.0304 MIN^(-1)` | |