Advertisements
Advertisements
प्रश्न
560ml of carbon monoxide is mixed with 500ml of oxygen and ignited. The chemicaI equation for the reaction is as folIows:
2CO + O2 → 2CO2
Calculate the volume of oxygen used and carbon dioxide formed in the above reaction.
उत्तर
2CO + O2 → 2CO2
From the reaction :
2 volumes of CO consumes = 1 volume of O2
So, 560ml of CO consumes = 112 x 560 = 280ml
Now, 2 volume of CO gives = 2 volume of CO2
So, 560ml of CO will give = 2 x 560 / 2 = 560ml
APPEARS IN
संबंधित प्रश्न
Each of the two flasks contains 2.0 g of gas at the same temperature and pressure. One flask contains oxygen and the other hydrogen. Which sample contains the greater number of molecules?
What volume of oxygen is required to burn completely a mixture of 22.4 dm3 of methane and 11 .2 dm3 of hydrogen in to carbon dioxide and steam? Equations of the reactions are given below:
CH4 + 2O2 → CO2 + 2H2O
2H2 + O2 → 2H2O
The equation 4NH35O2 → 4NO + 6H2O represents the catalytic oxidation of ammonia. If 100 cm3of ammonia is used, calculate the volume of oxygen required to oxidise the ammonia completely.
How much calcium oxide is formed when 82g of calcium nitrate is heated? Also find the volume of nitrogen dioxide evolved:
2Ca(NO3)2→ 2CaO + 4NO2 + O2 (Ca = 40,N = 14, O = 16)
Write the observation for the following:
Moist starch iodide paper is put on the mouth of a test tube containing chlorine gas.
Define atomicity of a gas. State the atomicity of Hydrogen, Phosphorus and Sulphur.
Calculate the volume of oxygen at STP required for the complete combustion of 100 litres of carbon monoxide at the same temperature and pressure.
\[\ce{2CO + O2 → 2CO2}\]
Solid ammonium dichromate decomposes as:
\[\ce{(NH4)2Cr2O7 -> N2 + Cr2O3 + 4H2O}\]
If 63 g of ammonium dichromate decomposes. Calculate the volume of N2 evolved at STP.
Given that the relative molecular mass of copper oxide is 80, what volume of ammonia (measured at STP) is required to completely reduce 120g of copper oxide? The equation for the reaction is:
\[\ce{3CuO + 2NH3 → 3Cu + 3H2O + N2}\]
Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide were collected at 27°C and normal pressure.
\[\ce{CaCO3 + 2HCl -> CaCl2 + H2O + CO2}\]
Calculate the mass of the acid required.
