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Question

Let order with respect to $A$ and $B$ are $\alpha$ and $\beta$ respectively.

$	herefore \frac{ dc }{ dt }= k [ A ]^\alpha[ B ]^\beta$

$1.2 	im

Vedclass · Accepted Answer

$\frac{dc}{dt} = k[A]$

Vedclass · Answer

Let order with respect to $A$ and $B$ are $\alpha$ and $\beta$ respectively.

$	herefore \frac{ dc }{ dt }= k [ A ]^\alpha[ B ]^\beta$

$1.2 	imes 10^{-3}= k [0.1]^\alpha[0.1]^\beta \quad...(i)$

$1.2 	imes 10^{-3}= k [0.1]^\alpha[0.2]^\beta \quad...(ii)$

$2.4 	imes 10^{-3}= k [0.2]^\alpha[0.1]^\beta \quad...(iii)$

Dividing $(ii)$ by $(i): 2^\beta=1 \quad 	herefore \beta=0$

Dividing $(iii)$ by $(i): 2^\alpha=2 \quad 	herefore \alpha=1$

Rate law will be: $\frac{ dc }{ dt }= k [ A ]$

Initial Conc. $(A)$	Initial Conc. $(B)$	Initial rate of formation of $C\,(mol\, L^-S^-)$
$0.1\,M$	$0.1\,M$	$1.2 \times 10^{-3}$
$0.1\,M$	$0.2\,M$	$1.2 \times 10^{-3}$
$0.2\,M$	$0.1\,M$	$2.4 \times 10^{-3}$

$A$ $(mol/l)$	$B$ $(mol/l)$	Rate
$0.05$	$0.05$	$1.2\times 10^{-3}$
$0.10$	$0.05$	$2.4\times 10^{-3}$
$0.05$	$0.10$	$1.2\times 10^{-3}$

Exp.	$[A]_0$	$[B]_0$	Initial rate
$(1)$	$0.012$	$0.035$	$0.10$
$(2)$	$0.024$	$0.070$	$0.80$
$(3)$	$0.024$	$0.035$	$0.10$
$(4)$	$0.012$	$0.070$	$0.80$

Expt. No.	$(A)$	$(B)$	Initial Rate
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

Similar Questions

Calculate the order of the reaction in $A$ and $B$

$A$

$(mol/l)$

$B$

$(mol/l)$
Rate

$0.05$   $0.05$ $1.2\times 10^{-3}$

$0.10$   $0.05$ $2.4\times 10^{-3}$

   $0.05$   $0.10$ $1.2\times 10^{-3}$

The data for the reaction $A + B \to C$ isThe rate law corresponds to the above data is

Exp.

$[A]_0$

$[B]_0$

Initial rate

$(1)$

$0.012$

$0.035$

$0.10$

$(2)$

$0.024$

$0.070$

$0.80$

$(3)$

$0.024$

$0.035$

$0.10$

$(4)$

$0.012$

$0.070$

$0.80$

Which among the following is a false statement

If in a certain reaction, two different reactants take part then

Select the rate law that corresponds to the data shown for the following reaction $A+ B\to C$

Expt. No. $(A)$ $(B)$ Initial Rate

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$
$0.024$
$0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

Similar Questions

Calculate the order of the reaction in $A$ and $B$ $A$ $(mol/l)$ $B$ $(mol/l)$ Rate $0.05$ $0.05$ $1.2\times 10^{-3}$ $0.10$ $0.05$ $2.4\times 10^{-3}$ $0.05$ $0.10$ $1.2\times 10^{-3}$

The data for the reaction $A + B \to C$ isThe rate law corresponds to the above data is Exp. $[A]_0$ $[B]_0$ Initial rate $(1)$ $0.012$ $0.035$ $0.10$ $(2)$ $0.024$ $0.070$ $0.80$ $(3)$ $0.024$ $0.035$ $0.10$ $(4)$ $0.012$ $0.070$ $0.80$

Which among the following is a false statement

If in a certain reaction, two different reactants take part then

Select the rate law that corresponds to the data shown for the following reaction $A+ B\to C$ Expt. No. $(A)$ $(B)$ Initial Rate $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

Calculate the order of the reaction in $A$ and $B$

$A$

$(mol/l)$

$B$

$(mol/l)$
Rate

$0.05$ $0.05$ $1.2\times 10^{-3}$

$0.10$ $0.05$ $2.4\times 10^{-3}$

$0.05$ $0.10$ $1.2\times 10^{-3}$

The data for the reaction $A + B \to C$ isThe rate law corresponds to the above data is

Exp.

$[A]_0$

$[B]_0$

Initial rate

$(1)$

$0.012$

$0.035$

$0.10$

$(2)$

$0.024$

$0.070$

$0.80$

$(3)$

$0.024$

$0.035$

$0.10$

$(4)$

$0.012$

$0.070$

$0.80$

Select the rate law that corresponds to the data shown for the following reaction $A+ B\to C$

Expt. No. $(A)$ $(B)$ Initial Rate

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$
$0.024$
$0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$