`40mL` gaseous mixture of `CO, CH_4 and Ne` was exploded with `10mL` of oxygen. After treatment with `KOH` the volume reduced by `9 mL`and again on treatment with alkaline pyrogallol, the volume further reduced by 1.5 mL. percentage of `CH_4` in the original mixture is :

20mL of a mixture of CO and H_(2) were mixed excess of O_(2) and exploded & cooled. There was a volume contraction of 18mL. All volume measurements corresponds to room temperature (27^(@)C) and one atmospheric pressure. Determine the volume ratio (V_(1):V_(2) "of" Co anf H_(2) in the original mixture .

CH4 reacts with Cl2 to form CH2Cl2 and HCl . calculate the volume of HCl formed when 80ml of methane reacts completely with Cl2.

The percentage by volume of C_(3)H_(8) in a gaseous mixture of C_(3)H_(8),CH_(4) and CO is 20. When 100mL of the mixture is burnt in excess of O_(2) the volume of CO_(2) produced is :

A mixture of 100ml of CO,CO_(2) and O_(2) was sparked. When the resulting gaseous mixture was passed through KOH solution, contraction in volume was found to be 80ml , the composition of initial mixture may be (in the same order)

A mixture of FeO and Fe_2 O_3 is completely reacted with 100mL of 0.25M acidified KMnO_4 solution. The resulting solution was then treated with Zn dust which converted Fe^(3+) of the solution to fe^(2+) . The Fe^(2=) required 100mL of 0.10MK_2 Cr_2O_7 solution. Find out the weight % Fe_2O_3 in the mixture.

25mL of 2N HCI, 50 mL of 4N HNO_3 and x mL of 2MH_2 SO_4 are mixed together and the total volume is made up to 1L after dilution. 50mL of this acid mixture completely reacted with 25mL of a 1NNa_2 CO_3 solution. The value of x is :

What volume of a liquid (in L) will contain 10 mole ? If molar mass of liquid is 280 and its density is 1.4 g/mL.

10 mL of H_(2)A (weak diprtic acid) solutio is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following obserbation is made Ip pH of the solution at first equivalence point is pH_(1) and at secnd equibalence point is pH_(2^.) Calculate the value of (pH_(2)-pH_(1)) at 25^(@)C Given for H_(2)A,pK_(a_1) =4.6 and pK_(a_2) =8, log 25=1.4

A mixture of H_(2)SO_(4) and H_(2)C_(2)O_(4) (oxalic acid ) and some inert impurity weighing 3.185 g was dessolved in water and the solution made up to 1litre. 10 mL of this solution required 3 mL of 0.1 N NaOH for complete neutralization. In another experiment 100 mL of the same solution in hot condition required 4 mL of 0.02 M KMnO_(4) solution for complete reaction. The mass % of H_(2)SO_(4) in the mixture was:

A volume of 12.5 mL of 0.05 M SeO_(2) reacts with 25 mL of 0.1 M CrSO_(4) which is oxidised to Cr^(3+) . To what oxidation state was the selenium converted by the reaction ?