Calculate the following:
The volume of unused oxygen when 200cc of ethane `[C_2 H_6 ]` is exploded with 2000cc of oxygen.

Calculate the following: The volume & number of moles of oxygen liberated at s.t.p. when 5.2 gm. of sodium peroxide [Na_2 O] reacts with water. 2Na_2 O_2 + 2H20 to 4NaOH + O_2 [Na=23, O=16]

The volume of oxygen liberated from 0.68g of H_(2)O_(2) is

1500 cm^(3) of oxygen was burnt with 300 cm^(3) of ethane (C_(2)H_(6)) . calculate the volume of unused oxygen.

The volume of oxygen liberated from 15 ml of 20 volume H_(2)O_(2) is

Calculate the number of oxygen atoms in 0.20 mole of Na_(2)CO_(3).10H_(2)O .

Calculate the total number of oxygen atoms present in 0.5 moles of H_(2)SO_(4)

Acetylene burns in air according to the reaction 2C_(2)H_(2) + 5O_(2) to4CO_(2) + 2H_(2)O at 100°C. Calculate the volume of air required to completely burn 50 cc of acetylene. (Air contains 20% oxygen by volume).

n- Butance (C_(4)H_(10)) is produced by monobromation of C_(2)H_(6) followed by the Wurtz reaction. Calculate the volume of ethane at STP requried to produce 55 g of n-butane. The bromination takes place with 90% yield and the Wurtz reaction with 85% yield.

In one mole of ethane (C_(2)H_(6)) , calculate the following: a. Number of moles of carbon atoms b. Number of moles of hydrogen stoms c. Number of molecules of ethane.

An organic compound contains carbon, hydrogen and oxygen. If the ratio percentage of C and H is 6:1 calculate the simplest formula of the compound, given that one molecule of the compound contains half as much oxygen as would be required to burn all the carbon and hydrogen atoms in it to CO_2 and H_2O