List of top Chemistry Questions on Chemical Kinetics asked in AP EAMCET

The following graph is obtained for a gas at different temperatures (T1, T2, T3). What is the correct order of temperature? (x-axis = velocity; y-axis = number of molecules)

The first order reaction \( A(g) \rightarrow B(g) + 2C(g) \) occurs at 25\(^\circ\)C. After 24 minutes the ratio of the concentration of products to the concentration of the reactant is 1:3. What is the half-life of the reaction (in min)? (log 1.11 = 0.046)
Given below are two statements
Statement - I: For isothermal irreversible change of an ideal gas, \[ q = -w = P_{\text{ext}}(V_{\text{final}} - V_{\text{initial}}) \] Statement - II: For adiabatic change, \[ \Delta U = W_{\text{adiabatic}} \] The correct answer is:

Observe the following stoichiometric equation
P4 + 3 OH- + 3 H2O → PH3 + 3 OH-.
What is the conjugate acid of OH- ?

A → P is a first order reaction. The following graph is obtained for this reaction. (x-axis = time; y-axis = conc. of A). The instantaneous rate of the reaction at point C is
first order reaction

A hydrocarbon containing C and H has 92.3% C. When 39 g of hydrocarbon was completely burnt in O2, x moles of water and y moles of CO2 were formed. x moles of water is sufficient to liberate 0.75 moles of H2 with Na metal. What is the weight (in g) of oxygen consumed?

RMS velocity of one mole of an ideal gas was measured at different temperatures. A graph of \( (u_{\text{rms}})^2 \) (on y-axis) and \( T/K \) (on x-axis) gave a straight line passing through the origin, and its slope is \( 249 \, \text{m}^2 \text{s}^{-2}\text{K}^{-1} \). What is the molar mass (in kg mol\(^{-1}\)) of the ideal gas? \(( R = 8.3 \, \text{J mol}^{-1} \text{K}^{-1} )\)

Identify the correct statements from the following:

For an ideal gas, the compressibility factor is 1.0.

The kinetic energy of NO (g) (molar mass = 30 g mol-1) at T(K) is \( x \) J mol-1. The kinetic energy of N2O4 (g) (molar mass = 92 g mol-1) at T(K) is \( 2x \) J mol-1.

The rate of diffusion of a gas is inversely proportional to the square root of its density.

 

At 298 K, for a first order reaction (A → P) the following graph is obtained. The rate constant (in s\(^{-1}\)) and initial concentration (in mol L\(^{-1}\)) of ‘A’ are respectively: 

Isomerisation of gaseous cyclobutane to butadiene is a first-order reaction. At \( T(K) \), the rate constant of the reaction is \( 3.3 \times 10^{-4} \, \text{s}^{-1} \). What is the time required (in min) to complete 90% of the reaction at the same temperature? (log 2 = 0.3)
The rate constant of a first order reaction was doubled when the temperature was increased from 300 to 310 K. What is its approximate activation energy (in kJ mol\(^{-1}\))?
(R = 8.3 J mol\(^{-1}\) K\(^{-1}\), \(\log 2 = 0.3\))

Given below are two statements:
Statement I: Viscosity of liquid decreases with an increase in temperature.
Statement II: The units of viscosity are kg m-1 s-2.

 At 300 K, for the reaction A → P, the ∆Ssys is 5 J K-1 mol-1. What is the heat absorbed (in kJ mol-1) by the system?

The rate constant for a zero order reaction \(A \rightarrow\) products is \(0.0030\ \mathrm{mol\ L^{-1}\ s^{-1}}\). How long will it take for the initial concentration of \(A\) to fall from \(0.10\ \mathrm{M}\) to \(0.075\ \mathrm{M}\)?