List of top Questions asked in AP EAPCET

In a series LCR circuit, the voltages across the capacitor, resistor, and inductor are in the ratio 2:3:6. If the voltage of the source in the circuit is 240 V, then the voltage across the inductor is
0.25 moles of $ \text{CH}_2\text{FCOOH} $ was dissolved in $ 0.5 \, \text{kg} $ of water. The depression in freezing point of the resultant solution was observed as $ 1^\circ \text{C} $. What is the van't Hoff factor? ($ K_f = 1.86 \, \text{K kg mol}^{-1} $)
A 1% (w/v) aqueous solution of a certain solute is isotonic with a 3% (w/v) solution of glucose (molar mass 180 g mol$^{-1}$). The molar mass of solute (in g mol$^{-1}$) is
At $T(K)$, the vapor pressure of water is $x$ kPa. What is the vapor pressure (in kPa) of 1 molal solution containing non-volatile solute?
Elements X and Y form two non-volatile compounds (XY and XY$_2$). When 10 g of XY is dissolved in 50 g of ethanol, the depression in freezing point ($\Delta T_f$) was 5.333 K. When 10 g of XY$_2$ is dissolved in 50 g of ethanol, the $\Delta T_f$ was 2.2857 K. What are the atomic weights of X and Y respectively?
($K_f = 2 \, \text{kg mol}^{-1}$)
248 g of ethylene glycol (C\(_2\)H\(_6\)O\(_2\)) is added to 200 g of water to prepare antifreeze. What is the molality of the resultant solution?
A solution containing 7.5 g of urea (molar mass = 60 g/mol) in 1 kg of water freezes at the same temperature as another solution containing 15 g of solute X in the same amount of water. The molar mass of X (g/mol) is
A centi molar solution of acetic acid is 50% dissociated at 27$^\circ$C. The osmotic pressure of the solution (in atm) is (R = 0.083 L atm K$^{-1}$ mol$^{-1}$)
At 300 K, vapour pressure of pure liquid A is 70 mm Hg. It forms an ideal solution with liquid B. Mole fraction of B = 0.2 and total vapour pressure of solution = 84 mm Hg. What is vapour pressure (in mm) of pure B?
An aqueous solution containing 0.2 g of a non-volatile solute 'A' in 21.5 g of water freezes at 272.814 K. If the freezing point of water is 273.16 K, the molar mass (in g mol$^{-1}$) of solute A is [K$_f$(H$_2$O) = 1.86 K kg mol$^{-1}$]
At T(K), the vapor pressure of x molal aqueous solution containing a non-volatile solute is 12.078 kPa. The vapor pressure of pure water at T(K) is 12.3 kPa. What is the value of x?
1.95 g of non-volatile and non-electrolyte solute dissolved in 100 g of benzene lowered the freezing point of it by 0.64 K. The molar mass of the solute (in g mol\(^{-1}\)) (\(K_f(\text{C}_6\text{H}_6) = 5.12 \, \text{K kg mol}^{-1}\)) is
A solution of urea in water has a boiling point of \( 100.18^\circ C \). What is the freezing point of the same solution, if \( K_f \) and \( K_b \) of water are \( 1.86 \) and \( 0.52 \) K kg mol\(^{-1} \), respectively? (Boiling point of water = \( 100^\circ C \))
At \( T \)(K), the vapour pressure of pure benzene and toluene are \( 75 \) and \( 22 \) mm Hg respectively. 23.4 g of benzene and 64.4 g of toluene are mixed to form an ideal solution. If the vapours are in equilibrium with the liquid mixture, the mole fraction of toluene in vapour phase is:
1.95 g of non-volatile and non-electrolyte solute dissolved in 100 g of benzene lowered the freezing point of it by 0.64 K. The molar mass of the solute (in g mol\(^{-1}\)) (\(K_f(\text{C}_6\text{H}_6) = 5.12 \, \text{K kg mol}^{-1}\)) is
At 298 K, 0.714 moles of liquid A is dissolved in 5.555 moles of liquid B. The vapour pressure of the resultant solution is 475 torr. The vapour pressure of pure liquid A at the same temperature is 280.7 torr. What is the vapour pressure of pure liquid B in torr?
A solution of urea in water has a boiling point of \( 100.18^\circ C \). What is the freezing point of the same solution, if \( K_f \) and \( K_b \) of water are \( 1.86 \) and \( 0.52 \) K kg mol\(^{-1} \), respectively? (Boiling point of water = \( 100^\circ C \))
At \( T \)(K), the vapour pressure of pure benzene and toluene are \( 75 \) and \( 22 \) mm Hg respectively. 23.4 g of benzene and 64.4 g of toluene are mixed to form an ideal solution. If the vapours are in equilibrium with the liquid mixture, the mole fraction of toluene in vapour phase is:
What is the approximate molality of 10% (w/w) aqueous glucose solution? (Molar mass of glucose = 180 g mol\(^{-1}\))
The van't Hoff factor for 0.5 m aqueous CH₃COOH solution is 1.075. What is the experimentally observed \(\Delta T_f\) (in K) for this solution? \( K_f = 1.86 \, \text{K kg mol}^{-1} \)
The following graph is obtained for an ideal solution containing a non-volatile solute. \(x\)- and \(y\)-axes represent, respectively
containing a non-volatile solute
Observe the following statements about dry cell:
It is a primary battery.
Zinc vessel acts as cathode.
A paste of moist \( \text{NH}_4\text{Cl}, \text{MnO}_2 \), and \( \text{ZnCl}_2 \) is present between two electrodes.
The potential of this cell is 1.5 V.
Match the following

The correct answer is:
Match the following:
List-I (Complex)List-II (Isomerism) 
A) [Co(NH3)5Br]SO4V) Ionization
B) [Co(en)3]3+I) Optical
C) [Co(NH3)5(NO2)]2+II) Linkage
D) [Co(NH3)3Cl3]III) Geometrical
In which of the following, complex ions are not in correct order with respect to their magnitude of crystal field splitting?