Rate of Reaction

Q. The rate constant for the reaction
$2N_2{O}_5\to 4N{O}_2+O_2$
is $3.0\times {10}^{-5}{\text{sec}}^{-1}$. If the rate is $2.4\times {10}^{-5}mol{L}^{-1}{\text{sec}}^{-1}$, then the concentration of $N_2{O}_5(inmole{L}^{-1}$) is

1. $1.4$
2. $1.2$
3. $0.004$
4. $0.8$

Q.

The average kinetic energy per molecule of ideal gas is equal to ____.

1. 

2. 

3. 

4. 

Q.

For the reaction $2\mathrm{A}+3\mathrm{B}+\left(3/2\right)\mathrm{C}\underset{}{\overset{}{\to }}3\mathrm{P}$, which statement is correct ?

1. $\raisebox{1ex}{$d{n}_A$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\raisebox{1ex}{$d{n}_B$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\raisebox{1ex}{$d{n}_C$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.$

2. $\raisebox{1ex}{$d{n}_A$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\left(\frac{3}{2}\right)\raisebox{1ex}{$d{n}_B$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\left(\frac{3}{4}\right)\raisebox{1ex}{$d{n}_C$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.$

3. $\raisebox{1ex}{$d{n}_A$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\left(\frac{2}{3}\right)\raisebox{1ex}{$d{n}_B$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\left(\frac{4}{3}\right)\raisebox{1ex}{$d{n}_C$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.$

4. $\raisebox{1ex}{$d{n}_A$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\left(\frac{2}{3}\right)\raisebox{1ex}{$d{n}_B$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.=\left(\frac{3}{4}\right)\raisebox{1ex}{$d{n}_C$}\!\left/ \!\raisebox{-1ex}{$dt$}\right.$

Q.

At $518°\mathrm{C},$ the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of $363$ $\mathrm{torr}$, was $1.00\mathrm{torr}{\mathrm{s}}^{-1}$when $5\%$ had reacted and $0.5\mathrm{torr}{\mathrm{s}}^{-1}$ when $33\%$ had reacted. The order of the reaction is

1. $3$

2. $1$

3. $0$

4. $2$

Q. Tde is 15. Compute the mass in grams of KCIO3 necessary to produce 67.2 litres of oxygen at S.T.P. according to the reaction 2KCIO3 (s)2KCI (s) + 302 (g) [Molecular weight of KCIO3 122.5] ed in - (2) 2 (1) 96 (4) 245 (3) 122.5

Q.

The average kinetic energy of an ideal gas per molecule in SI units at 25${}^{\circ }$C will be

1. 6.17×10⁻²¹ kJ

2. 6.17×10⁻²¹ J

3. 6.17×10⁻²⁰ J

4. 7.16×10⁻²⁰ J

Q. X2 +Y2 = 2XY reaction was studied at a certain temperature . in the beginning 1 mole of X2 was taken in a one litre flask and 2 moles of Y2 was taken in another 2 litre flask .what is the equilibrium concentration of X2 and Y2 ? (given equilibrium conc. of \lbrack XY\rbrack =0.6 mol/l)

Q. A reaction follows the given concentration (M)-time graph. The rate for this reaction at 20 seconds will be

1. $4\times {10}^{-3}M/s$
2. $8\times {10}^{-2}M/s$
3. $2\times {10}^{-2}M/s$
4. $7\times {10}^{-3}M/s$

Q.

An oxidation-reduction reaction in which $3$ electrons are transferred has a $∆{\mathrm{G}}^0$ of $17.37{\mathrm{KJmol}}^{-1}$ at ${25}^0\mathrm{C}$. The value of ${{\mathrm{E}}^0}_{\mathrm{cell}}$ (in $\mathrm{V}$) is ______ $\times {10}^{-2}$. $(1\mathrm{F}=96500{\mathrm{Cmol}}^{-1})$

Q. 24. In Victor Meyers Method, 0.2 gm of an organic compound displaced 56 mL of air at S.T.P. The molecular weight of compound is

Q. Nitrogen tetra oxide $\left(N_2{O}_4\right)$ decomposes as $N_2{O}_4\left(g\right)\to 2N{O}_2\left(g\right)$. If the pressure of $\left(N_2{O}_4\right)$ falls from 0.50 atm to 0.32 atm is 30 minutes, the rate of appearance of $N{O}_2\left(g\right)$ is

1. 0.006 atm/min
2. 0.003 atm/min
3. 0.012 atm/min
4. 0.024 atm/min

Q.

Calculate the time taken in seconds for $40\%$ completion of a first order reaction, if its rate constant is $3.3\times {{10}^{-4}}^{}{{\sec }^{-1}}^{}.$

Q. 35. 116 mg of a compound on vaporisation in a Victor Meyers apparatus displaces 44.8 ml of air measured at STP. The molecular weight of the compound is A. 116 B. 232 C. 58 D. 44.8

Q. 5.at 273 k and 1 atm. , 10 lt of N2O4 decomposes to NO2. what is the degree of dissociation when the original volume is 25% less than that of existing volume?

Q. Comprehension Iodine is an impor†an t subs†an ce needed by the body of a human being. We consume it in the form of salt, which has very very samll % con†an t of I_2. Iodine has various industrial application also. The following process has been used to obtain iodine from oil field brines in California: NaI+AgNO_3=AgI+NaNO_3 AgI+Fe=Fe+Ag FeI_2+Cl_2=FeCl_3+I_2 Q. If 381 kg of iodine is produced per hour, 40kg then mass of AgNO_3 required per hour will be: (A) 170kg (B) 340kg (C) 255kg (D) 510kg Q. If above reaction is carried out by taking 150kg of NaI and 85kg of AgNO_3, then number of moles of iodine formed is: (A) 0.5 (B) 500 (C) 250 (D) 0.25

Q. Compute the mass in grams of KCIO necessary toproduce 67.2 litres of oxygen at S.T.P. according tothe reaction2KCI (s) +302 (g)2KCIO3 (s)\lbrack Molecular weight of-KCIO, = 122.5\rbrack3

Q. Percentage of oxygen in a compound is 0.8% by weight then the minimum molecular weight of compound will be?

Q. 12. Assertion: molar mass of a volatile organic compound is determined by Victor meyers method reason: molar mass of a non volatile organic compound is determined by ebullioscopy

Q. For a reaction, $N_2{O}_5⟶2N{O}_2+\frac{1}{2}{O}_2$
Given:
$\frac{-d\left[N_2{O}_5\right]}{dt}=k_1\left[N_2{O}_5\right]$
$\frac{d\left[N{O}_2\right]}{dt}=k_2\left[N_2{O}_5\right]$
$\frac{d\left[O_2\right]}{dt}=k_3\left[N_2{O}_5\right]$
The relation between $k_1,k_2$ and $k_3$ are:

1. $2k_1=k_2=4k_3$
2. $k_1=k_2=k_3$
3. $2k_1=4k_2=k_3$
4. $\frac{1}{2}{k}_1=k_2=\frac{1}{4}{k}_3$

Q. 58. THE RATE CONSTANT FOR FORWARD AND BACKWARD REACTIONS OF HYDROLYSIS OF ESTER ARE 1.1*10 RAISE TO -2 AND 1.5*10 RAISE TO -3 PER MINUTE RESPECTIVELY. EQUILIBRIUM CONSTANT FOR THE REACTION IS CH3COOC2H5 + H2O ->CH3COOH + C2H5OH

Q. The active mass of 7.0gof nitrogen ia2.0L container would be??

Q. Oxidation state of sulphur in sodium tetrathionate $\left(N{a}_2{S}_4{O}_6\right)$ is

1. $+2$
2. $+1.5$
3. $+4$
4. $+2.5$

Q. For the reaction 2A + B + C $\to A_{2}B$ + C the rate law is found to be Rate =k[A][B]${}^2$ with $k=2\times {10}^{-6}mo{l}^{-2}{L}^2{s}^{-1}$
The initial rate of reaction with $\left[A\right]=0.1mol{L}^{-1},\left[B\right]=0.2mol{L}^{-1}and\left[C\right]=0.8mol{L}^{-1}$ is

1. $6.4\times {10}^{-8}mol{L}^{-1}{s}^{-1}$
2. $4\times {10}^{-3}mol{L}^{-1}{s}^{-1}$
3. $8\times {10}^{-9}mol{L}^{-1}{s}^{-1}$
4. $4\times {10}^{-7}mol{L}^{-1}{s}^{-1}$

Q. $xA+yB\to zC.If-\frac{d\left[A\right]}{dt}=-\frac{d\left[B\right]}{dt}=1.5\frac{d\left[C\right]}{dt}$ then x.y and z are

1. 1, 1, 1
2. 3, 2, 3
3. 3, 3, 2
4. 2, 2, 3

Q. For the reaction $2A+B\to C$, the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is:

$\left[A\right]\left(mol{L}^{-1}\right)$	$\left[B\right]\left(mol{L}^{-1}\right)$	$\text{Initial Rate}\left(mol{L}^{-1}{s}^{-1}\right)$
0.05	0.05	0.045
0.10	0.05	0.090
0.20	0.10	0.72

1. Rate = $k\left[A{]}^2\right[B{]}^2$
2. Rate = $k\left[A\right][B{]}^2$
3. Rate = $k\left[A\right]\left[B\right]$
4. Rate = $k\left[A{]}^2\right[B]$

Q.

For the reaction$\underset{\mathrm{dinitrogen}\mathrm{pentaoxide}}{\underbrace{2{\mathrm{N}}_2{\mathrm{O}}_5\left(\mathrm{g}\right)}}\to \underset{\mathrm{Nirogen}\mathrm{dioxide}}{\underbrace{4{\mathrm{NO}}_2\left(\mathrm{g}\right)}}+\underset{\mathrm{Oxygen}}{\underbrace{{\mathrm{O}}_2\left(\mathrm{g}\right)}}$, if the initial concentration of ${\mathrm{N}}_2{\mathrm{O}}_5$is $7.2{\mathrm{mol}}^{-1}$ and after $20$minutes, ${\mathrm{NO}}_2$ becomes $2.4{\mathrm{mol}}^{-1}$, then what will be the rate of decomposition of ${\mathrm{N}}_2{\mathrm{O}}_5$ in ${\mathrm{mol}}^{-1}{\min }^{-1}$$?$

Q. The initial rate of hydrolysis methyl acetate (1 M) by a weak acid (HA, 1M) is 1/100th of that of a strong acid (HX, 1M), at 25°C. The Ka of HA is?

Q. The mass of N2 required to produce 10 g of NH3 from the reaction is N2 + 3H2 → 2NH3

Q. Choose the correct option regarding order and molecularity:

Q. When dragons burn their victims, the following reaction takes place:

$2C+O_2⟶2C{O}_2$

The average rate of reaction could be expressed as?

1. 
2. 
3. 
4. All of the above