For the reaction: `aA + bB rarr cC+dD` Rate `= (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt)` In the following reaction, `xA rarr yB` `log.[-(d[A])/(dt)] = log.[(d[B])/(dt)] + 0.3` where negative isgn indicates rate of disappearance of the reactant. Thus, `x:y` is:A. `1:2`B. `2:1`C. `3:1`D. `3:10`

For the reaction: `aA + bB rarr cC+dD` Rate `= (dx)/(dt) = (-1)/(a)(d[

1.	For the reaction: `aA + bB rarr cC+dD` Rate `= (dx)/(dt) = (-1)/(a)(d[A])/(dt) = (-1)/(b)(d[B])/(dt) = (1)/( c)(d[C])/(dt) = (1)/(d)(d[D])/(dt)` In the following reaction, `xA rarr yB` `log.[-(d[A])/(dt)] = log.[(d[B])/(dt)] + 0.3` where negative isgn indicates rate of disappearance of the reactant. Thus, `x:y` is:A. `1:2`B. `2:1`C. `3:1`D. `3:10`
Answer» Correct Answer - B `xA rarr yB` `(-d[A])/(x dt) = (1)/(y) (d[B])/(dt)` `log.((-d[A])/(dt)) = log.(d[B])/(dt) + log.(x)/(y)` `:. log.((x)/(y)) = 0.3` `:. (x)/(y) = 2` or `x:y = 2:1`

Discussion

No Comment Found

Related InterviewSolutions

Rate law for the reaction `A + 2B rarr C`, is found to be Rate = k [A] [B]. If the concentration of reactant B is doubled keeping the concentration of A constant, the value of rate constant will beA. the sameB. doubledC. quadrupledD. halved
Which of the following statements is incorrect about the collision theory of chemicacl reaction ?A. It considers reacting molecules or atoms to be hard spheres and ignores their structrual features.B. Number of effective collisions determines the rate of reaction.C. Collision of atoms or molecules processig sufficient thereshold energy results into the product formation.D. Molecules should collide with sufficient threshold energy andproper orientatin for the collision to be effective.
A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be `k_(1) and k_(2)` respectively. ThenA. `k_(2)=0.25 k_(1)`B. `k_(2)=0.5k_(1)`C. `k_(2)=4k_(1)`D. `k_(2)=2k_(1)`
The half-life of a reaction is halved as the initial concentration of the reaction is doubled. The order of the reaction isA. 0.5B. 1C. 2D. 0
75 % of first order reaction is complete in 30 minutes. What is the time required for 93.75 % of the reaction (in minutes) ?A. 45B. 120C. 90D. 60
A reaction is 50 % complete in 2 hours and 75 % complete in 4 hours the order of reaction is
A certain zero order reaction has `k = 0.025 M s^(-1)` for the disappearance of `A`. What will be the concentration of `A` after `15` seconds if the initial concentration is `0.5 M` ?A. `0.5M`B. `0.32M`C. `0.12M`D. `0.06M`
If the concentration is mentioned in mol `L^(-1)` units and time in seconds, what are the units of k for zero order reaction and first order reaction?
Average rate of reaction does not give the true picture of the reaction rate. Explain.
Rate constant k of a reaction is dependent on temperatur: `k=Ae^(Ea//RT)` K has the least value atA. high T and high `E_(a)`B. high T and small `E_(a)`C. low T and low `E_(a)`D. low T and high `E_(a)`

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment