For the hypothetical reaction,
`A rarr` Products, rate `=-k[A]`
The negative sign used in the rate expression indicate that
Correct Answer - D Draw energy profile diagram
2 Answers 1 viewsCorrect Answer - C `CH_(3)CH_(2)CH_(2)Cl overset(alc. KOH)rarr CH_(3)CH=CH_(2) overset(HBr)rarr CH_(3)-underset(Br)underset("| ")("C ")H-CH_(3)overset(Na)underset("ether")rarr underset("2,3-Dimethylbutane")(CH_(3)-overset(CH_(3))overset("| ")("C ")H-overset(CH_(3))overset("| ")("C ")H-CH_(3))`
2 Answers 1 viewsCorrect Answer - C `HC-=CHoverset(H_(2)"O"//Hg^(2+))underset(H_(2)SO_(4))rarrH_(3)C-overset(O)overset(||)underset((X))C-H` `overset(LiAlH_(4))rarrH_(3)C-underset((Y))("CH"_(2))-OHoverset(P_(4)//Br_(2))rarrunderset("Ethyl bromide")(C_(2)H_(5)Br)`
2 Answers 1 viewsrate = `k[A][B]^(2)` By reducing the volume to `1/3` of its original volume, the concentration of the reactants will become three times. `therefore` rate = `k[3A][3B]^(2)=27k[A][B]^(2)` ltbr. Hence, the reaction...
2 Answers 1 viewsa) The rate law epression is: Rate(r) = `k[A]^(1//3)[B]^(2)therefore` Order of reaction `=1/3 + 2=2(1/3)` b) Rate constant, k =`("rate")/([A]^(1//3)[B]^(2))` `therefore` Units of rate constant = `(moldm^(-3)s^(-1))/((mol dm^(-3^(1//3))(mol dm^(-3))^(2)))` `=(moldm^(-3))^(1-7//3)s^(-1)=(mol...
2 Answers 1 viewsIn an elementary reaction, the number of atoms or ions which are colliding to react is known as molecularity. Had the reaction been of elementary nature (single step reaction) the...
2 Answers 1 viewsCorrect Answer - A a) The value of rate constant depends upon temperature and not upon the initial concentration of reactants and products.
2 Answers 1 viewsFrom expts. (2) and (3) , it is clear that when concentration of A is kept constant and that of B is doubled, the rate increasefour times. This shows that...
2 Answers 1 views`A" "+ " "OH^(-)" "rarr` Products `t=0 " " 0.002 " "0.3` `k=(2.303)/(30xx(0.002-03))log_(10).(0.3[0.002-(0.002xx1)/(100)])/(0.002[0.3-(0.002xx1)/(100)])` `k=1.12xx10^(-3)"litre" "mol"^(-1)s^(-1)`
2 Answers 1 viewsCorrect Answer - A For zero order reaction, x=kt `:. (a)/(2)=kxxt_(1//2),i.e.,t_(1//2)=(a)/(2k)" ".....(i)` For frist order reaction, `t_(1//2)=(log_(e)2)/(k)" ".....(ii)` From eqs. (i) and (ii), `(a)/(2k)=(log_(e)2)/(k)` `a=log_(e)4M`
2 Answers 1 views