Following is the rate constant of reaction what is the overall order of reaction ?
$(a)$ $6.66 \times 10^{-3} \,s ^{-1}$
$(b)$ $4.5 \times 10^{-2} \,mol ^{-1} \,L \,s ^{-1}$
Following is the rate constant of reaction what is the overall order of reaction ?
$(a)$ $6.66 \times 10^{-3} \,s ^{-1}$
$(b)$ $4.5 \times 10^{-2} \,mol ^{-1} \,L \,s ^{-1}$
Similar Questions
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iv)$ $C _{2} H _{5} Cl ( g ) \rightarrow C _{2} H _{4}( g )+ HCl ( g ) \quad$ Rate $=k\left[ C _{2} H _{5} Cl \right]$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iv)$ $C _{2} H _{5} Cl ( g ) \rightarrow C _{2} H _{4}( g )+ HCl ( g ) \quad$ Rate $=k\left[ C _{2} H _{5} Cl \right]$
The reaction, $X + 2Y + Z \to N$ occurs by the following mechanism
$(i)$ $X + Y \rightleftharpoons M$ very rapid equilibrium
$(ii)$ $M + Z \to P$ slow
$(iii)$ $O + Y \to N$ very fast
What is the rate law for this reaction
The reaction, $X + 2Y + Z \to N$ occurs by the following mechanism
$(i)$ $X + Y \rightleftharpoons M$ very rapid equilibrium
$(ii)$ $M + Z \to P$ slow
$(iii)$ $O + Y \to N$ very fast
What is the rate law for this reaction
In the following reaction $A \to B + C$, rate constant is $0.001\, M/sec$. If we start with $1M$ of $A$, the conc. of $A$ & $B$ after $10$ min are respectively
In the following reaction $A \to B + C$, rate constant is $0.001\, M/sec$. If we start with $1M$ of $A$, the conc. of $A$ & $B$ after $10$ min are respectively
Which of the following is correct ?
Which of the following is correct ?
Which of these does not influence the rate of reaction
Which of these does not influence the rate of reaction