List of top Questions asked in AP EAPCET- 2023

A, B and C are weak acids. Their dissociation constants ($K_a(A)$, $K_a(B)$, $K_a(C)$) are \[ 3.5 \times 10^{-4}, 1 \times 10^{-5} \text{ and } 5 \times 10^{-10} \text{ respectively. The pH of 1L of 0.01 M each of these solutions follow the order.} \]

Observe the following solutions \[ \text{I. Black coffee} \quad \text{II. 0.2M NaOH} \quad \text{III. Lemon juice} \quad \text{IV. Lime water} \quad \text{V. Human Saliva} \quad \text{VI. Tomato juice} \] The number of solutions having pH range of 1-7 and 7-14, in the above list, is respectively

The rate constant, k for a first order reaction, $ \text{C}_2\text{H}_5\text{I}(g) \rightarrow \text{C}_2\text{H}_4(g) + \text{HI}(g) $ is $ x \, \text{s}^{-1} $ at 600 K and $ 4x \, \text{s}^{-1} $ at 700 K. The energy of activation of the reaction (in kJ mol$ ^{-1} $) is (log 4 = 0.6, R = 8.3 J K$ ^{-1} $ mol$ ^{-1} $)

The auto catalyst in the redox reaction involving acidified potassium permanganate and oxalic acid is

A reaction, 3X(g) $\rightarrow$ 2Y(g) + Z(g) takes place in a closed vessel. What is the rate of formation of Y (in mol L$^{-1}$ s$^{-1}$) if the rate of disappearance of X is 7.2 $\times$ 10$^{-3}$ mol L$^{-1}$ s$^{-1}$?

A first-order reaction has the rate constant of $1.15 \times 10^{-3} \, \text{s}^{-1}$. The time required to reduce 10 g of reactant to 6 g is $x \times 10^2$ sec. What is the approximate value of $x$?

Consider the reaction carried out at T(K):
$\text{A(g) + B(g) → C(g)}$
$\text{The rate law for this reaction is \(r = k[A]^2[B]^2$}\). The concentration of A in experiment 2 and rate in experiment 3 shown as $x$ and $z$ in the table. $x$ and $z$ are respectively:\[\begin{array}{|c|c|c|c|} \hline \text{Experiment} & [A]~(\text{mol L}^{-1}) & [B]~(\text{mol L}^{-1}) & \text{Initial rate (mol L}^{-1} \text{s}^{-1}) \\ \hline 1 & 0.05 & 0.05 & R \\ 2 & x & 0.05 & 2R \\ 3 & 0.20 & 0.10 & z\\ \hline \end{array}\]

Given below are two statements
Assertion (A): A catalyst generally increases the rate of a reaction
Reason (R): It lowers the activation energy of a reaction by providing a new path

The rate constant, $ k $, of a zero order reaction $ 2 \text{NH}_3 (g) \xrightarrow{P_{1130K}} \text{N}_2 (g) + 3 \text{H}_2 (g) $ is $ y \times 10^{-4} \, \text{mol} \, \text{L}^{-1} \, \text{s}^{-1} $. The rate of formation of hydrogen (in mol L$^{-1}$ s$^{-1}$) is

Given below are two statements
Assertion (A) : Protium and deuterium differ in their rates of reactions
Reason (R) : They have different enthalpies of bond dissociation The correct answer is

If the standard enthalpy change ($\Delta H^o$) for reaction \[ \text{H}_2(g) + \text{Br}_2(l) \rightarrow 2 \text{HBr}(g) \] is $-72.8 \, \text{kJ}$, the standard enthalpy of formation ($\Delta H_f^o$) of $\text{HBr}(g)$ in $\text{kJ mol}^{-1}$ is:

At $ T(K) $, the equilibrium constant for $ A (g) \rightleftharpoons B (g) $ is $ 10^2 $. If the rate of forward reaction is 0.025 mol L$^{-1}$ s$^{-1}$, the rate of backward reaction (in mol L$^{-1}$ s$^{-1}$) is

20 mL of 0.1 M HCl is added to 30 mL of 0.1 M NaOH. To this solution, extra 50 mL of water was added. What is the molarity of the final solution formed?

If the time required for 40% completion of a first order reaction is 50 minutes, what is the time required for completion of 80% of the same reaction?
($ \log 2 = 0.3010, \log 5 = 0.6990, \log 6 = 0.7782 $)

At T(K), the $K_p$ for the reaction $A_2B_6(g) \rightleftharpoons 2A_2B_4(g) + B_2(g)$ is 0.04 atm. The equilibrium pressure (in atm) of $A_2B_6(g)$ when it is placed in a flask at 4 atm pressure and allowed to come to above equilibrium is

One mole of $ A (g) $ is heated to $ T(K) $ till the following equilibrium is obtained \[ A(g) \rightleftharpoons B(g) \] The equilibrium constant of this reaction is $ 10^{-1} $. After reaching the equilibrium, 0.5 moles of A (g) is added and heated. The equilibrium is again established. The value of $ \left[\frac{A}{B}\right] $ is

Observe the following species \[ \text{AlCl}_3, \, \text{NH}_3, \, \text{H}^+, \, \text{Co}^{3+}, \, \text{OH}^-, \, \text{H}\text{Mg}^{2+}, \, \text{BF}_3, \, \text{Cl}^- \] How many Lewis bases are present in the above list?

Observe the following equilibrium $$\text{Fe}^{3+}(aq) + \text{SCN}^-(aq) \rightleftharpoons [\text{Fe(SCN)}]^{2+}(aq)$$ yellow \hspace{1cm colourless \hspace{1cm} deep red}
Addition of aqueous oxalic acid solution to the above equilibrium

Given below are two statements
Statement I: The changes in pH with temperature are so small that we often ignore it
Statement II: When the hydrogen ion concentration changes by a factor of 100, the pH changes by one unit
In the light of above statements, identify the correct answer from the options given below