The stability of carbanions in the following:
 
is in the order of:

1.  (1) > (2) > (3) > (4)

2.  (2) > (3) > (4) > (1)

3.  (4) > (2) > (3) > (1)

4.  (1) > (3) > (2) > (4)

The dissociation equilibrium of a gas AB₂ can be represented as 
 $2A{B}_2\left(g\right)$ $\leftrightharpoons$ $2AB\left(g\right)$ $+$ $B_2\left(g\right)$ $$
The degree of dissociation is ‘x’ and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant K_P and total pressure p is:
1. (2KP/p)
2. (2Kp /p)^1/3
3. (2KP/p)^1/2
4. (KP/P)

Which one of the following statements is not true?

In the given hydrocarbon, 

The type/state of hybridization of carbons 1, 3, and 5 respectively are:

1. sp², sp, sp³

2. sp, sp³, sp²

3. sp, sp², sp³

4. sp³, sp², sp

The value of K_P1 and K_p2 for the reactions
 $X$ $\leftrightharpoons$ $Y$ $+Z$ $......\left(i\right)$
$and$ $A$ $\leftrightharpoons 2B$ $......\left(ii\right)\hspace{0.17em}$
are in the ratio of 9 : 1. If the degree of dissociation of X and A is equal, then the total pressure at equilibrium(i) and (ii) are in the ratio:

In DNA, the complementary bases are:

1. Adenine and thymine; guanine and cytosine

2. Adenine and thymine; guanine and uracil

3. Adenine and guanine, thymine and cytosine

4. Uracil and adenine; cytosine and guanine

The bromination of acetone occurring in an acid solution is represented by the equation. 
CH₃COCH₃(aq)+ Br₂(aq) → 
CH₃COCH₂Br(aq) + H⁺(aq) + Br^-(aq) 

The kinetic energy data were obtained for given reaction concentrations. 
Initial concentrations, M 
 $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$   $\left[{\mathrm{Br}}_2\right]$    $\left[{\mathrm{H}}^{+}\right]$

   0.30             0.05      0.05

   0.30             0.10      0.05

   0.30             0.10      0.10

   0.40             0.05      0.20
Initial rate, the disappearance of Br₂, Ms^-1 
5.7 $\times$ 10^-5

5.7 $\times$  10^-5

1.2 $\times$ 10^-4

3.1 $\times$ 10^-4
Based on the above data, the rate of the equation is:

1. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$ $\left[{\mathrm{H}}^{+}\right]$

2. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[\mathrm{CH}={\mathrm{COCH}}_3\right]$ $\left[{\mathrm{Br}}_2\right]$

3. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$ $\left[{\mathrm{Br}}_2\right]$ ${\left[{\mathrm{H}}^{+}\right]}^2$

4. $\mathrm{Rate}$ $=$ $\mathrm{k}$ $\left[{\mathrm{CH}}_3{\mathrm{COCH}}_3\right]$ $\left[{\mathrm{Br}}_2\right]$ $\left[{\mathrm{H}}^{+}\right]$

Find the equilibrium constant for the reaction:

H₂(g) + I₂(g) ⇌ 2HI(g)

Given that:

HI(g) ⇌ ½H₂(g) + ½I₂(g)  K = 8