In which of the following cases, does the reaction go farthest to completion
In which of the following cases, does the reaction go farthest to completion
- A
$K = {10^3}$
- B
$K = {10^{ - 2}}$
- C
$K = 10$
- D
$K = 1$
Similar Questions
For the reaction $A + B \to $ products, what will be the order of reaction with respect to $A$ and $B$ ?
Exp.
$[A]\,(mol\,L^{-1})$
$[B]\,(mol\,L^{-1})$
Initial rate $(mol\,L^{-1}\,s^{-1})$
$1.$
$2.5\times 10^{-4}$
$3\times 10^{-5}$
$5\times 10^{-4}$
$2.$
$5\times 10^{-4}$
$6\times 10^{-5}$
$4\times 10^{-3}$
$3.$
$1\times 10^{-3}$
$6\times 10^{-5}$
$1.6\times 10^{-2}$
For the reaction $A + B \to $ products, what will be the order of reaction with respect to $A$ and $B$ ?
| Exp. | $[A]\,(mol\,L^{-1})$ | $[B]\,(mol\,L^{-1})$ | Initial rate $(mol\,L^{-1}\,s^{-1})$ |
| $1.$ | $2.5\times 10^{-4}$ | $3\times 10^{-5}$ | $5\times 10^{-4}$ |
| $2.$ | $5\times 10^{-4}$ | $6\times 10^{-5}$ | $4\times 10^{-3}$ |
| $3.$ | $1\times 10^{-3}$ | $6\times 10^{-5}$ | $1.6\times 10^{-2}$ |
The rate law for the reaction below is given by the expression $k\left[ A \right]\left[ B \right]$
$A + B \to$ Product
If the concentration of $B$ is increased from $0.1$ to $0.3\, mole$, keeping the value of $A$ at $0.1\, mole$, the rate constant will be
The rate law for the reaction below is given by the expression $k\left[ A \right]\left[ B \right]$
$A + B \to$ Product
If the concentration of $B$ is increased from $0.1$ to $0.3\, mole$, keeping the value of $A$ at $0.1\, mole$, the rate constant will be
- [JEE MAIN 2016]
Write the rate equation for the reaction $2A + B\to C$ if the order of the reaction is zero.
Write the rate equation for the reaction $2A + B\to C$ if the order of the reaction is zero.
Write unit of rate constant of following reaction :
$1.$ fourth order
$2.$ third order
Write unit of rate constant of following reaction :
$1.$ fourth order
$2.$ third order
In a reaction between $A$ and $B$, the initial rate of reaction $\left(r_{0}\right)$ was measured for different initial concentrations of $A$ and $B$ as given below:
$A/mol\,\,{L^{ - 1}}$
$0.20$
$0.20$
$0.40$
$B/mol\,\,{L^{ - 1}}$
$0.30$
$0.10$
$0.05$
${r_0}/mol\,\,{L^{ - 1}}\,\,{s^{ - 1}}$
$5.07 \times 10^{-5}$
$5.07 \times 10^{-5}$
$1.43 \times 10^{-4}$
What is the order of the reaction with respect to $A$ and $B$?
In a reaction between $A$ and $B$, the initial rate of reaction $\left(r_{0}\right)$ was measured for different initial concentrations of $A$ and $B$ as given below:
| $A/mol\,\,{L^{ - 1}}$ | $0.20$ | $0.20$ | $0.40$ |
| $B/mol\,\,{L^{ - 1}}$ | $0.30$ | $0.10$ | $0.05$ |
| ${r_0}/mol\,\,{L^{ - 1}}\,\,{s^{ - 1}}$ | $5.07 \times 10^{-5}$ | $5.07 \times 10^{-5}$ | $1.43 \times 10^{-4}$ |
What is the order of the reaction with respect to $A$ and $B$?