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प्रश्न
Differentiate between 2H and H2
उत्तर
| 2H | H2 |
| 2H corresponds to two atoms of Hydrogen element. | H2 corresponds to a hydrogen olecule which contains two atoms of hydrogen . |
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संबंधित प्रश्न
Oxygen oxidises ethyne to carbon dioxide and water as shown by the equation:
\[\ce{2C2H2 + 5O2 -> 4CO2 + 2H2O}\]
What volume of ethyne gas at STP required to produce 8.4 dm3 of carbon dioxide at STP?
[H = 1, C = 12, O = 16]
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
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.
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)
The ratio between the number of molecules in 2g of hydrogen and 32 g of oxygen is
[Given that H=1,O=16]
Solid ammonium dichromate decomposes as:
\[\ce{(NH4)2Cr2O7 -> N2 + Cr2O3 + 4H2O}\]
If 63 g of ammonium dichromate decomposes. Calculate what will be the loss of mass.
What mass of copper hydroxide is precipitated by using 200 gm of sodium hydroxide?
\[\ce{2NaOH + CuSO4 -> Na2SO4 + Cu(OH)2↓}\]
[Cu = 64, Na = 23, S = 32, H = 1]
Solve the following numerical problem:
Ethane burns in oxygen according to the chemical equation:
\[\ce{2C2H6 + 7O2 -> 4CO2 + 6H2O}\]
If 80 ml of ethane is burned in 300 ml of oxygen, find the composition of the resultant gaseous mixture when measured at room temperature.
66g of ammonium sulphate is produced by the action of ammonia on sulphuric acid. Write a balanced equation and calculate the mass of acid required.
Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
\[\ce{P + 5HNO3_{(conc.)}-> H3PO4 + H2O + 5NO2}\]
If 9.3 g of phosphorus was used in the reaction, calculate:
- Number of moles of phosphorus taken.
- The mass of phosphoric acid formed.
- The volume of nitrogen dioxide produced at STP.
