In a gaseous reaction
${A_{2\left( g \right)}} \longrightarrow {B_{\left( g \right)}} + \frac{1}{2}\,{C_{\left( g \right)}}$ the increase in pressure from $100\, mm$ to $120\, mm$ is noticed in $5\,\min$. The rate of dissappearence of $A_2$ in $mm\, min^{-1}$ is
In a gaseous reaction
${A_{2\left( g \right)}} \longrightarrow {B_{\left( g \right)}} + \frac{1}{2}\,{C_{\left( g \right)}}$ the increase in pressure from $100\, mm$ to $120\, mm$ is noticed in $5\,\min$. The rate of dissappearence of $A_2$ in $mm\, min^{-1}$ is
- A
$4$
- B
$8$
- C
$16$
- D
$2$
Similar Questions
Consider the reaction between chlorine and nitric oxide
$Cl _{2}( g )+2 NO ( g ) \rightarrow 2 NOCl ( g )$
On doubling the concentration of both reactants, the rate of the reaction increases by a factor of $8 .$ However, if only the concentration of $C l_{2}$ is doubled, the rate increases by a factor of $2 .$ The order of this reaction with respect to $NO$ is :
Consider the reaction between chlorine and nitric oxide
$Cl _{2}( g )+2 NO ( g ) \rightarrow 2 NOCl ( g )$
On doubling the concentration of both reactants, the rate of the reaction increases by a factor of $8 .$ However, if only the concentration of $C l_{2}$ is doubled, the rate increases by a factor of $2 .$ The order of this reaction with respect to $NO$ is :
- [NEET 2017]
What is the order of reaction' for $A + B \to C$
Observation
$[A]$
$[B]$
Rate of reaction
$1$
$0.1$
$0.1$
$2\times10^{-3}\, mol\, L^{-1}\,sec^{-1}$
$2$
$0.2$
$0.1$
$0.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$
$3$
$0.1$
$0.2$
$1.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$
What is the order of reaction' for $A + B \to C$
| Observation | $[A]$ | $[B]$ | Rate of reaction |
| $1$ | $0.1$ | $0.1$ | $2\times10^{-3}\, mol\, L^{-1}\,sec^{-1}$ |
| $2$ | $0.2$ | $0.1$ | $0.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$ |
| $3$ | $0.1$ | $0.2$ | $1.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$ |
If the rate constant $(K)$ of a reaction is $1.6 \times 10^{-3}\, mol\, L^{-1}\, min^{-1}$ the order of reaction is
If the rate constant $(K)$ of a reaction is $1.6 \times 10^{-3}\, mol\, L^{-1}\, min^{-1}$ the order of reaction is
For the reaction $A \to B$, the rate law expression is : Rate $ = \,k\,[A]$ Which of the following statements is incorrect
For the reaction $A \to B$, the rate law expression is : Rate $ = \,k\,[A]$ Which of the following statements is incorrect
In a reaction, the concentration of reactant is increased two times and three times then the increases in rate of reaction were four times and nine times respectively, order of reaction is
In a reaction, the concentration of reactant is increased two times and three times then the increases in rate of reaction were four times and nine times respectively, order of reaction is