NEET UG Chemistry — Physical Chemistry previous year questions with solutions.
Match List I with List II.  Choose the correct answer from the options given below:
For the following reaction at 300 K $\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})$ the enthalpy change is +15 kJ then the internal energy change is:
Rate constants of a reaction at 500 K and $700 \mid \mathrm{K}$ are $0.04 \mathrm{~s}^{-1}$ and $0.14 \mathrm{~s}^{-1}$, respectively; then, activation energy of the reaction is : (Given: $\log 3.5=0.5441, \mathrm{R}=8.31 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$
The energy of an electron in the ground state $(n=1)$ for $\mathrm{He}^{+}$ion is $-x J$, then that for an electron in $n=2$ state for $\mathrm{Be}^{3+}$ ion in J is
Which plot of $\ln k$ vs $\frac{1}{\mathrm{~T}}$ is consistent with Arrhenius equation?
Match List-I with List-II:  Choose the correct answer from the options given below:
In which of the following processes entropy increases? A. A liquid evaporates to vapour. B. Temperature of a crystalline solid lowered from 130 K to 0 K . C. $2 \mathrm{NaHCO}_{3(\mathrm{~s})} \rightarrow \mathrm{Na}_2 \mathrm{CO}_{3(\mathrm{~s})}+\mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$ D. $\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{Cl}_{(\mathrm{g})}$ Choose the correct answer from the options given below:
Consider the following reaction in a sealed vessel at equilibrium with concentrations of $\mathrm{N}_2=3.0 \times 10^{-3} \mathrm{M}, \mathrm{O}_2=4.2 \times 10^{-3} \mathrm{M}$ and $\mathrm{NO}=2.8 \times 10^{-3} \mathrm{M}$. $2 \mathrm{NO}_{(\mathrm{g})} \rightleftharpoons \mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$ If 0.1 mol $\mathrm{L}^{-1}$ of $\mathrm{NO}_{(\mathrm{g})}$ is taken in a closed vessel, what will be degree of dissociation ( $\alpha$ ) of $\mathrm{NO}_{(\mathrm{g})}$ at equilibrium?
For the reaction $2 \mathrm{~A} \rightleftharpoons \mathrm{B}+\mathrm{C}, \mathrm{K}_{\mathrm{C}}=4 \times 10^{-3}$. At a given time, the composition of reaction mixture is: $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=2 \times 10^{-3} \mathrm{M}$. Then, which of the following is correct?
The rate of a reaction quadruples when temperature changes from $27^{\circ} \mathrm{C}$ to $57^{\circ} \mathrm{C}$. Calculate the energy o activation. Given $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \log 4=0.6021$
For an endothermic reaction: (A) $\mathrm{qp}_{\mathrm{p}}$ is negative. (B) $\Delta_r H$ is positive. (C) $\Delta_r \mathrm{H}$ is negative. (D) $\mathrm{q}_{\mathrm{p}}$ is positive. Choose the correct answer from the options given below:
Which indicator is used in the titration of sodium hydroxide against oxalic acid and what is the colour change at the end point?
Match List I with List II  Choose the correct answer from the options given below :
For the reaction in equilibrium $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}), \Delta \mathrm{H}=-\mathrm{Q}$ Reaction is favoured in forward direction by:
The highest number of helium atoms is in
The quantum numbers of four electrons are given below : I. $n=4 ; I=2 ; m_1=-2 ; s=-\frac{1}{2}$ II. $n=3 ; I=2 ; m_1=1 ; s=+\frac{1}{2}$ III. $n=4 ; I=1 ; m_1=0 ; s=+\frac{1}{2}$ IV. $n=3 ; I=1 ; m_1=-1 ; s=+\frac{1}{2}$ The correct decreasing order of energy of these electrons is
The amount of glucose required to prepare 250 mL of $\frac{\mathrm{M}}{20}$ aquepus solution is : (Molar mass of glucose : $180 \mathrm{~g} \mathrm{~mol}^{-1}$ )
Which of the following plot represents the variation of $\ln \mathrm{k}$ versus $\frac{1}{T}$ in accordance with Arrhenius equation?
Which reaction is NOT a redox reaction?
Following data is for a reaction between reactants A and B :  The order of the reaction with respect to $A$ and $B$, respectively, are
Match List I with List II.  Choose the correct answer from the options given below:
The Henry's law constant $\left(\mathrm{K}_H\right)$ values of three gases $(\mathrm{A}, \mathrm{B}, \mathrm{C})$ in water are $145,2 \times 10^{-5}$ and 35 kbar , respectively. The solubility of these gases in water follow the order:
1.0 g of $\mathrm{H}_2$ has same number of molecules as in:
Activation energy of any chemical reaction can be calculated if one knows the value of