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0.6 L of an ideal gas weighs 1.80 g at 27^(@)C and 1 atm pressure. Its approximate molar mass is :

0.6 g of a solute is dissolved in 0.1 littre of a solvent which develops an osmotic pressure of 1.23 atm at 27^(@)C. The molecular mass of the substance is

0.5g of a nonvolatile organic compound (mol.wt. 65) is dissolved in 100mL of "CC"l_(4). If the vapour pressure of pure "CC"l_(4) is 143 mm, what would be the vapour pressure of the solution? (Density of "CC"l_(4) solution is 1.58g//"cc")

0.596g of a gaseous compound containing only boron and hydrogen occupies 484 mL at NTP. When the compound was ignited in excess of oxygen, all its hydrogen was recovered as 1.17g of H_(2)O and all the boron was present as B_(2)O_(3). Find the molecular formula of the compound (B=10.8, H=1)

0.58 g of hydrocarbon on combustion gave 0.9 g water. The percentage of carbon is about :

0.53 gm of Na_(2)CO_(3) has been dissolved in 100 ml of a sodium carbonate solution. The normality of the solution will be

0.5 normal solution of a salt placed between two platnum electrodes 2.0 cm. apart and of area of cross section 4.0 sq. cm. has a resistance of 25 ohms. Calculate the equivalent conductivity of solution.

0.5 mole of SO_2 gas at 27^@C is expanded in reversible adiabatic condition to make volume 8 times.Final temperature (in K) and work done by gas (in Cal) respectively are x and y.Report your answer as y/x. (Take ideal behaviour of gas, R=2 Cal/K mol and 2^(1.2)=2.3)

0.5 mole of electron is passed though two electrolytic cells in series. One contains silber ions, and the other zinc ions. Assume that only cathode reaction in each cell is the reduction of the ion to the metal. How many gm of each metals will be deposited.

0.5 mole of eachH_(2),SO_(2) and CH_(4) are kept in a container. A holewas made in the container. After 3 hours, the order of partial pressures in the container will be

0.5moleof anidealmonoatomic gas atSTP conditionsundergoes a process, if the finalvolumeof gas is(22.5xxe) lit,then theentropy change in thid processin k/J/mol is .(Given: Processisobaric ) (Fill your answerby multiplyingit with (100)/(R))

0.5 mole each of two ideal gases A(C_(v)=3/2R)andB=(C_(v)=5/2R) are taken in a container and expanded reversibly and adiabatically from V = 1 L to V = 4 L starting from initial temperature T = 300 K. Find DeltaH for the process in (cal/mol).

0.5 mole each of H_(2), SO_(2) & CH_(4) are kept in container. A hole was made in the container. After 3 hours the order of partial pressures in the container will be:

0.5 molar NaCl and 0.8 molal urea solutions are formed to be isotonic at 27^(@)C then the degree of dissociation of NaCl under these consitions is reported as xxx10% . What is the value of 'x' ?

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) of water is 1.86 K kg "mol"^(-1) , the lowering in freezing point of the solution is :

0.5 mol of H_(2)SO_(4) is mixed with 0.2 mol of Ca(OH)_(2) . The maximum number of moles of CaSO_(4) formed is

0.5 mol of BaCl_2is mixed with 0.2 mol ofNa_3PO_4 . The maximum number of mol of Ba_3(PO_4)_2that can be formed is :

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86 K kg mol^(-1), the lowering in freezing point of solution will be :

0.5 mol each of H_(2), SO_(2) and CH_(4) are ketp in a container. A hole was made in the container. After 3 hours, the order of partial pressure in the container will be :

0.5 M glucose solution is iso-osmotic with which of the following solutions ?

0.5 M ammonium benzoate is hydrolyzed to 0.25 percent, hence its hydrolysis constant is

0.5 L of 1.0 M NaCl solution is electrolysed for 965 a using a current of 5 ampere. What will be the pH of the solution after the electrolysis?

0.5 gm of an oxalate was dissolved in water and the solution raised to 100 ml. 10 ml of this solution when titrated with N/20 KMnO_4 required 10 ml of KMnO_4. Calculate the % of oxalate ion in the sample. (K = 39, Mn = 55)

0.5 g of NaOH is required by 0.4 gm of a polybasic acid H_(n)A (Molecular weight = 96 gm) for complete neutralisation .Value of 'n' would be : (Assume all H atom are replaced )-

0.5 g of metal nitrate gave 0.43 g of metal sulphate

0.5 g of KCl was dissolved in 100 g of water and the solution originally at 20^@C froze at - 0.24^@C. Calculate the percentage dissociation of salt.Given : K_ffor water = 1.86 K kg/mol, At, mass : K= 39 u, Cl = 35.5 u.

0.5 g of fuming H_(2)SO_(4) (oleum ) is diluted with water . The solution is completely neutralised by 26.7 mL of 0.4 N naOH .Find the percentage of free SO_(3) in the sample of oleum.

0.5 g of fuming H_(2)SO_(4) (oleum) is diluted with water. The solution requires 26.7 ml of 0.4 N NaOH for complete neutralization. Find the % of free SO_(3) in the sample of oleum.

0.5 g of an organic compound containing nitrogen on Kjeldahlising required 29 mL of N/5H_2SO_4 for complete neutralisation of ammonia. The percentage of nitrogen in the compound is :

0.5 g KCl was dissolved in 100 g water and the solution originally at 20^(@)C, froze at -0.24^(@)C. Calculate the percentage ionization of salt. K_(f) per 1000 g of water =1.86^(@)C.

0.5 F of electric current was passed through 5 molar solution of AgNO_(3), CuSO_(4) " and " AlCl_(3) connected in series. Find out the concentration of each of the electrolyte after the electrolysis.

0.5 F of electric current was passed though 5 molar solutions of AgNO_(3), CuSO_(4) and AlCl_(3) connected in series. Find out the concentration of each of the electrolyte after the electrolysis ?

A sample of 0.50 g of an organic compound was treated according to Kjeldahl’s method. The ammonia evolved was absorbed in 50 ml of 0.5 M H_(2)SO_(4). The residual acid required 60 mL of 0.5 M solution of NaOH for neutralisation. Find the percentage composition of nitrogen in the compound.

0.4g of an organic compound gave 0.188g of silver bromide by a halogen estimation method. The percentage of bromine in the compound is : (at.mass of Ag=108, Br=80) :

0.48 g of a volatile substance upon vapourisation gives 112 ml vapours at STP. Ratio of rate of diffusion of vapours of volatile substance to H_2(g) is (assume vapours behave ideally)

0.465g of an organic compound upon combustion produced 1.32g of CO_(2) and 0.315g of H_(2)O. 0.2325g of the same compound gave 27.8 mL of dry N_(2) at NTP. If the compound contained C, H and N find its formula

0.46 g ofan organic compound containing C,H oxygen was heatedstronglyin steam of N_(2) gas . The gaseous mixture thus obtained was passed over heated coke at 1373 K and then passed through warm solution of iodine pentoxide when 2.54 g of iodine. The percentage of O_(2) in the compound is

0.45g of a dibasic organic acid upon combustion produced 0.44g of CO_(2) and 0.09g of H_(2)O. 0.76g of its silver salt when ignited gave 0.54g of pure silver. What is the fomula of the acid? (Ag=108)

0.45 g of an acid of molecular weight 90 was neutralised by 20 mL of 0.5 N caustic potash .The basicity of the acid is

0.45 g of an acid ( mol. Mass = 90 ) is neutralised by 20 mol of 0.5 N NaOH solution. The basicity of the acid is :

0.45 g an acid (mol wt.=90) required 20 ml of 0.5 N KOH for complete neutralization. Basicity of acid is

0.44 g of a monohydric alcohol when added to methylmagnesium iodide in ether liberates at S.T.P.,112 cm^(3) of methane. With PCC the same alcohol forms a carbonyl compound that answers silver mirror test. The monohydric alcohol is

0.440 g of a substance dissolved in 22.2 g of benzene lowered the freezing point of benzene by 0.567^(@)C. The molecular mass of the substance (K_(f)=5.12^(@)kg C mol^(-1))

0.44 g of a monohydric alcohol when added to methyl magnesium iodide in ether liberates at STP 112 cm^3 of methane with PCC the same alcohol form a carbonyl compound that answers silver mirror test. Identify the compound.

0.44 g of a monohydric alcohol when added to methyl magnesium iodide in ether lilberates at STP 112 cm^(3) of methane with PCC the same alcohol form a carbonyl compound that answers silver mirror test. Identify the compound.

0.44 g of a hydrocarbon on complete combustion with oxygen gave 1.8g water and 0.88 g carbon dioxide. Show that these resutls are in asccordance with the law of conservation of mass.