Which of the following statements is false ?
Which of the following statements is false ?
- A
For an endothermic reaction, energy of product is greater than that of reactant
- B
The rate law for a reaction depends on the concentrations of all reactant that appear in the stoichiometric equation.
- C
The rate of a zero order reaction is independent of the concentration of the catalyst.
- D
The specific rate constant for a reaction is independent of the concentrations of the reacting species
Similar Questions
For a reaction $A+ B\to $ Products, the rate law is - Rate $=$ $k\,[A]\, [B]^{\frac {3}{2}}$ . Can the reaction be an elementary reaction ? Explain.
For a reaction $A+ B\to $ Products, the rate law is - Rate $=$ $k\,[A]\, [B]^{\frac {3}{2}}$ . Can the reaction be an elementary reaction ? Explain.
For the reaction $A \to B$, the rate increases by a factor of $2.25 $ when the concentration of $A$ is increased by $ 1.5$. What is the order of the reaction
For the reaction $A \to B$, the rate increases by a factor of $2.25 $ when the concentration of $A$ is increased by $ 1.5$. What is the order of the reaction
For the following rate law determine the unit of rate constant. Rate $=-\frac{d[ R ]}{d t}=k[ A ]^{\frac{1}{2}}[ B ]^{2}$
For the following rate law determine the unit of rate constant. Rate $=-\frac{d[ R ]}{d t}=k[ A ]^{\frac{1}{2}}[ B ]^{2}$
For the reaction $2NO_2 + F_2 \to 2NO_2F$, following mechanism has been provided :
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + {F_2}\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as
For the reaction $2NO_2 + F_2 \to 2NO_2F$, following mechanism has been provided :
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + {F_2}\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as
The half-life of $2 $ sample are $0.1 $ and $ 0.4 $ seconds. Their respective concentration are $200 $ and $ 50 $ respectively. What is the order of the reaction
The half-life of $2 $ sample are $0.1 $ and $ 0.4 $ seconds. Their respective concentration are $200 $ and $ 50 $ respectively. What is the order of the reaction