How can you determine the rate law of the following reaction ?
$2NO\,(g) + O_2\,(g)\to 2NO_{2} \,(g)$
How can you determine the rate law of the following reaction ?
$2NO\,(g) + O_2\,(g)\to 2NO_{2} \,(g)$
The rate law can be determined by 'measuring the rate of this reaction as a function of initial concentration by keeping the concentration of one of the reactants constant and changing the concentration of other reactant or by changing the concentration dependance of rate, rate law can be determined.
Example : If the concentration of $\mathrm{NO}$ is doubled, keeping the concentration of oxygen continously, the process velocity four time. Which accelerate, so the rate $=k[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right]$ and the introduction of the acceleration rule is as follows.
Similar Questions
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$
Initial $[A_2]$
Initial $[B_2]$
$R.O.R.\,(r)\,Ms^{-1}$
$0.2$
$0.2$
$0.04$
$0.1$
$0.4$
$0.04$
$0.2$
$0.4$
$0.08$
Order of reaction with respect to $A_2$ and $B_2$ are respectively
${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$
| Initial $[A_2]$ | Initial $[B_2]$ | $R.O.R.\,(r)\,Ms^{-1}$ |
| $0.2$ | $0.2$ | $0.04$ |
| $0.1$ | $0.4$ | $0.04$ |
| $0.2$ | $0.4$ | $0.08$ |
Order of reaction with respect to $A_2$ and $B_2$ are respectively
The specific rate constant of a first order reaction depends on the
The specific rate constant of a first order reaction depends on the
- [IIT 1981]
In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$ torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$
In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$ torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$
For the decomposition of azoisopropane to hexane and nitrogen at $543$ $K ,$ the following data are obtained.
$t$ $(sec)$
$P(m m \text { of } H g)$
$0$
$35.0$
$360$
$54.0$
$720$
$63.0$
Calculate the rate constant.
For the decomposition of azoisopropane to hexane and nitrogen at $543$ $K ,$ the following data are obtained.
| $t$ $(sec)$ | $P(m m \text { of } H g)$ |
| $0$ | $35.0$ |
| $360$ | $54.0$ |
| $720$ | $63.0$ |
Calculate the rate constant.