Hydrogen and oxygen combine to form `H_2 O_2 and H_2 O` containing `5.93% and 11.2%` hydrogen respectively. The data illustrates :

Oxidation state of oxygen in H_2O_2 is

Oxidation state of oxygen in H_(2)O_(2) is

H_(2)O_(2) acts both as oxidant and reductant. H_(2)O and O_(2) are products when H_(2)O_(2) acts as oxidant and reductant respectively. The strength of H_(2)O_(2) is expressed in terms of molarity, normality, % strength and volume strength. H_(2)O_(2) decomposes as H_(2)O_(2)rarrH_(2)+1//2O_(2)(g) i.e., one mole O_(2) is released from 2 mole H_(2)O_(2) .x. .volume. strength of H_(2)O_(2) means 1 volume (mL or litre) of H_(2)O_(2) sample released x volume (mL or litre) O_(2) gas at NTP on its decomposition. Hence molarity = x//11.2 moles per litre, i.e., normality of H_(2)O_(2)=x//5.6 Thus volume strength, i.e., x=5.6xx Normality. Weigth of H_(2)O_(2) (in gm) present in 100 mL H_(2)O_(2) solution is called percentage strength of H_(2)O_(2) How much volume of H_(2)O_(2) solution of 22.4 .vol. strength is required to oxidise 6.3 gm oxalic acid

Balance the equation: H_2O_2 to H_2O+O_2

Hydrogen combines with oxygen to form H_(2)O in which 16 g of oxygen combine with 2g of hydrogen . Hydrogen also combines with carbon to form CH_(4) in which 2 g of hydrogen combine with 6 g of carbon . If carbon and oxygen combine together then they will do show in the ratio of

Compare the structures of H_(2)O and H_(2)O_(2)

Catalytic union of H_2 and O_2 to get H_2O_2 is found in

The standard enthalpies of formation of H_(2)O_(2(l)) and H_(2)O_((l)) are -187.8kJ "mole"^(-1) and -285.8 kJ "mole"^(-1) respectively. The DeltaH^(0) for the decomposition of one mole of H_(2)O_(2(l)) " to" H_(2)O_((l)) and O_(2(g)) is

The percentage of CH_(2)O in CuSO_(4)5H_(2)O is