Arrhenius Equation

Q.

A graph is plotted for a real gas which follows Van der Waals equation with $P{V}_m$ taken on y-axis and P on x-axis. Find the intercept of the line where $V_m$ is the molar volume.

1. 

2. 

3. 

4. 

Q. the rate constant for first order decomposition if certain reaction is described by the equation log k = 9.27-7.2×10^-3K/T the activation energy of reaction is ​

Q.

In Born-Haber cycle, the sum of the enthalpy changes around a cycle is

1. Constant

2. Zero

3. Positive integer

4. Negative integer

Q. 55 In a reversible reaction, the forward reaction was 3 time faster than that of reverse reaction. The reaction quotient is _______

Q. For the plot of $lnk\text{versus}1/T$ of Arrhenius equation, the slope and y-intercept are respectively.

Q. how to determine n factor of reaction c5h12 +o2=co2+ h2

Q. For a non-spontaneous reaction at all temperatures the correct set of thermodynamic parameter is

1. $\Delta H=-ve$
   $\Delta S=+ve$
2. $\Delta H=+ve$
   $\Delta S=-ve$
3. $\Delta H=+ve$
   $\Delta S=+ve$
4. $\Delta H=-ve$
   $\Delta S=-ve$

Q.

The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be:

$(R=8.314J{K}^{-1}mo{l}^{-1}andlog2=0.301)$

(IIT-JEE-2013)

1. $48.6kJmo{l}^{-1}$

2. $58.5kJmo{l}^{-1}$

3. $60.5kJmo{l}^{-1}$
4. $53.6kJmo{l}^{-1}$

Q. For gaseous reaction, following data is given:
$A\to B,k_1={10}^{15}{e}^{-2000/T}$
$C\to D,k_2={10}^{14}{e}^{-1000/T}$
The temperature at which $k_1=k_2$ is:

Q. Milk turns sour at ${40}^{\circ }$C three times as faster as $0^{\circ }$C. Hence, $E_a$ in the process of turning of milk sour is

1. $\frac{2.303\times 2\times 313\times 273}{40}log3$
2. $\frac{2.303\times 2\times 313\times 273}{40}log\left(1/3\right)cal$
3. $\frac{2.303\times 2\times 40}{273\times 313}log3cal$
4. $Noneofthese$

Q. Let’s assume you are a student of Arrhenius. He asked you to calculate $E_a$ for a reaction so that he can study a reaction on which he is working for a long time. He told you the rate constants of the reaction at 500 K and 700 K are $0.02s^{-1}and0.07s^{-1}$ respectively. Calculate the value of $E_a$.

1. 18231 J
2. 12831 J
3. 18431 J
4. 19231 J

Q. 47. I2_2I is a reversible reaction . which factor will favour forward reaction A_increase in concentration of 2I B_increase in temperature C_both a, b D_Decrease in concentration of I2 Given delta Hfor reaction is +150

Q. A first order reaction occuring at 300 K has an activation energy of 2.484 $kcal/mol$. When the temperature is doubled then the rate of the reaction is increased by n times. Find the value of n. (Take ln 2 = 0.69 and R = 2 $cal/mol.K$)

Q.

Let’s assume I want to double the rate of a reaction. The constraint is that I can only increase the temperature by 10 K. Calculate the minimum activation energy required if the temperature is 300K.

1. $54kJmo{l}^{-1}$

2. $64kJmo{l}^{-1}$

3. $94kJmo{l}^{-1}$

4. $84kJmo{l}^{-1}$

Q. The energy of activation of a first order reaction is $187.06kJmo{l}^{-1}$ at 750 K and the value of pre-exponential factor A is $1.97\times {10}^{12}{s}^{-1}$. Calculate the half life. $(e^{-30}=9.35\times {10}^{-14})$

1. 9.76s
2. 5.76s
3. 8.76s
4. 3.76s

Q. Let’s assume you are a student of Arrhenius. He asked you to calculate $E_a$ for a reaction so that he can study a reaction on which he is working for a long time. He told you the rate constants of the reaction at 500 K and 700 K are $0.02s^{-1}and0.07s^{-1}$ respectively. Calculate the value of $E_a$.

1. 18231 J
2. 12831 J
3. 18431 J
4. 19231 J

Q.

For a first order reaction A ⟶ P, the temperature (T) dependent rate constant (k) was found to follow the equation log k = -2000(1/T) + 6.0. The pre-exponential factor A and the activation energy $E_a,$ respectively, are

(IIT-JEE, 2009)

1. $1.0\times {10}^6{s}^{-1}and9.2kJmo{l}^{-1}$

2. $6.0s^{-1}and16.6kJmo{l}^{-1}$

3. $1.0\times {10}^6{s}^{-1}and16.6kJmo{l}^{-1}$

4. $1.0\times {10}^6{s}^{-1}and38.3kJmo{l}^{-1}$

Q. A first order reaction is $50\%$ complete in $30$ minutes at $27{}^{\circ }C$ and in 10 minutes at $47{}^{\circ }C$. The energy of activation $E_a$ of the reaction is:
$(log2=0.3,log3=0.5,R=\frac{25}{3}J{K}^{-1}mo{l}^{-1})$

1. 46 $kJmo{l}^{-1}$
2. 35 $kJmo{l}^{-1}$
3. 84 $kJmo{l}^{-1}$
4. 30 $kJmo{l}^{-1}$

Q. For the reaction $A\to B$, the rate constant $k\left({\text{s}}^{-1}\right)$ is given by

${\text{log}}_{10}k=20.35-\frac{(2.47\times {10}^3)}{T}$

The energy of activation in ${\text{kJ mol}}^{-1}$ is
(Nearest integer)

[Given : R=8.314 ${\text{JK}}^{-1}{\text{mol}}^{-1}$]

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