Chemistry
Water decomposes to O2 and H2 under suitable conditions as represented by the equation below: 2H2O 2H2 + O2 (a) If 2500 cm3 of H2 is produced, what volume of O2 is liberated at the same time and under the same conditions of temperature and pressure? (b) The 2500 cm3 of H2 is subjected to times increase in pressure (temp. remaining constant). What volume will H2 now occupy? (c) Taking the volume of H2 calculated in 5(b), what changes must be made in Kelvin (absolute) temperature to return the volume to 2500 cm3 pressure remaining constant.
Related Questions
112 cm3 of H2S (g) is mixed with 120 cm3 of Cl2 (g) at STP to produce HCl (g) and sulphur (s). Write a balanced equation for this reaction and calculate
(i) the volume of gaseous product formed
(ii) composition of the resulting mixture
1250 cc of oxygen was burnt with 300 cc of ethane [C2H6]. Calculate the volume of unused oxygen and the volume of carbon dioxide formed:
2C2H6 + 7O2 ⟶ 4CO2 + 6H2O
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CH4 + 2Cl2 ⟶ CH2Cl2 + 2HCl
What volume of propane is burnt for every 500 cm3 of air used in the reaction under the same conditions? (assuming oxygen is 1/5th of air)
C3H8 + 5O2 ⟶ 3CO2 + 4H2O