Which is correct about zero order reaction
Which is correct about zero order reaction
- A
Rate of reaction depends on decay constant
- B
Rate of reaction is independent of concentration
- C
Unit of rate constant is concentration$^{ - 1}$
- D
Unit of rate constant is concentration$^{ - 1}$ time$^{ - 1}$
Similar Questions
Hydrolysis of methyl acetate in aq. solution has been studied by titrating the liberated acetic acid against solidum hydroxide. The conc. of the ester at different time is given below :
Time $(t)$ $\min$
$0$
$30$
$60$
$90$
Con. of ester
$(C)$
$0.850$
$0.800$
$0.754$
$0.710$
Show that it follows a pseudo first order reaction as the conc. of $H_2O$ remain nearly constant $(54.2\,mol\,L^{-1})$ during the course of the reaction. What is the value of $k'$ in this reaction ?
Hydrolysis of methyl acetate in aq. solution has been studied by titrating the liberated acetic acid against solidum hydroxide. The conc. of the ester at different time is given below :
| Time $(t)$ $\min$ | $0$ | $30$ | $60$ | $90$ |
| Con. of ester $(C)$ |
$0.850$ | $0.800$ | $0.754$ |
$0.710$ |
Show that it follows a pseudo first order reaction as the conc. of $H_2O$ remain nearly constant $(54.2\,mol\,L^{-1})$ during the course of the reaction. What is the value of $k'$ in this reaction ?
The half life for second order reaction is $30\, minutes$. If the initial concentration is $0.1\, M$ then the value of rate constant will be ............ $M^{-1}\, min^{-1}$
The half life for second order reaction is $30\, minutes$. If the initial concentration is $0.1\, M$ then the value of rate constant will be ............ $M^{-1}\, min^{-1}$
The formation of gas at the surface of tungsten due to adsorption is the reaction of order
The formation of gas at the surface of tungsten due to adsorption is the reaction of order
- [AIEEE 2002]
Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$
take place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{{slow}} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{{fast}} H_2O + Br_2$
The order of the reaction is
Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to Br_2 + 2H_2O$
take place in two steps :
$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{{slow}} HOBr + H_2O$
$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{{fast}} H_2O + Br_2$
The order of the reaction is
Write differential rate expression of following reaction and give its order of reaction :
$2 N _{2} O _{5} \rightarrow 4 NO _{2}( g )+ O _{2}$
$C _{4} H _{9} Cl + OH ^{-} \rightarrow C _{4} H _{9} OH + Cl ^{-}$
Write differential rate expression of following reaction and give its order of reaction :
$2 N _{2} O _{5} \rightarrow 4 NO _{2}( g )+ O _{2}$
$C _{4} H _{9} Cl + OH ^{-} \rightarrow C _{4} H _{9} OH + Cl ^{-}$