For a particular reaction, the rate expression is given as $r = k[A] [B]^{0.5}$. If the volume of vessel is reduced to one-fourth of the initial volume, the rate of reaction would
For a particular reaction, the rate expression is given as $r = k[A] [B]^{0.5}$. If the volume of vessel is reduced to one-fourth of the initial volume, the rate of reaction would
- A
decrease $1/4\ times$
- B
increased by $8\ times$
- C
decreased by $1/8\ times$
- D
remains unaffected
Similar Questions
For the reaction : $2A + B \to A_2B$ ; the rate $= K[A]\, [B]^2$ with $K = 2.0\times10^{-6}\, lit^2\, mol^{-2}\, sec^{-1}$. Initial concentration of $A$ and $B$ are $0.2\, mol/lit$ and $0.4\, mol/lit$ respectively. Calculate the rate of reaction after $[A]$ is reduced to $0.12\, mol/litre$.
For the reaction : $2A + B \to A_2B$ ; the rate $= K[A]\, [B]^2$ with $K = 2.0\times10^{-6}\, lit^2\, mol^{-2}\, sec^{-1}$. Initial concentration of $A$ and $B$ are $0.2\, mol/lit$ and $0.4\, mol/lit$ respectively. Calculate the rate of reaction after $[A]$ is reduced to $0.12\, mol/litre$.
For the reaction, $2A + B\,\to $ products , when the concentrations of $A$ and $B$ both were doubled, the rate of the reaction increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $2.4 \,mol\,L^{-1}\,s^{-1}.$ When the concentration of $A$ alone is doubled, the rate increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $0.6\,mol\,L^{-1}\,s^{-1}.$ Which one of the following statements is correct?
For the reaction, $2A + B\,\to $ products , when the concentrations of $A$ and $B$ both were doubled, the rate of the reaction increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $2.4 \,mol\,L^{-1}\,s^{-1}.$ When the concentration of $A$ alone is doubled, the rate increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $0.6\,mol\,L^{-1}\,s^{-1}.$ Which one of the following statements is correct?
- [JEE MAIN 2019]
The order of a reaction which has the rate expression $\frac{{dc}}{{dt}} = K{[E]^{3/2}}{[D]^{3/2}}$ is
The order of a reaction which has the rate expression $\frac{{dc}}{{dt}} = K{[E]^{3/2}}{[D]^{3/2}}$ is
A study of chemical kinetics of the reaction $A + B \to$ Products, gave the following data at $25\,^oC$.
Exp. No.
[A]
[B]
Rate
$1.$
$1.0$
$0.15$
$4.2 × 10^{-6}$
$2.$
$2.0$
$0.15$
$8.4 × 10^{-6}$
$3.$
$1.0$
$0.20$
$5.6 × 10^{-6}$
Find out rate law
A study of chemical kinetics of the reaction $A + B \to$ Products, gave the following data at $25\,^oC$.
| Exp. No. | [A] | [B] | Rate |
| $1.$ | $1.0$ | $0.15$ | $4.2 × 10^{-6}$ |
| $2.$ | $2.0$ | $0.15$ | $8.4 × 10^{-6}$ |
| $3.$ | $1.0$ | $0.20$ | $5.6 × 10^{-6}$ |
Find out rate law
Which one of the following statements for the order of a reaction is incorrect?
Which one of the following statements for the order of a reaction is incorrect?
- [AIPMT 2011]