Advertisements
Advertisements
प्रश्न
Nitrogen and hydrogen react to form ammonia.
\[\ce{N2_{(g)} + 3H2_{(g)}-> 2NH3_{(g)}}\]
If 1000g of H2 reacts with 2000g of N2.
Calculate the mass of ammonia (NH3) that will be formed.
उत्तर
28 g of N2 forms NH3 = 34 g
2000 g of N2 forms NH3 = `34/28 xx 2000`
= 2428.6 g
संबंधित प्रश्न
Nitrogen and oxygen gas react as illustrated by the equation given below: N2 + O2 → 2NO
Calculate the volume of each reacting gas required to produce 1400cm3 of nitric oxide.
Samples of the gases O2, N2, CO2 and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of Oxygen, occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure :
What is the volume occupied by : X molecules of N2.
Samples of the gases O2, N2, CO2 and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of Oxygen, occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure :
What is the volume occupied by : 3X molecules of CO? [C=12,N=14,O=16]
The equation for the burning of octane is:
\[\ce{2C8H18 + 25O2 -> 16CO2 + 18H2O}\]
What volume, at STP, is occupied by 8 moles?
O2 is evolved by heating KCIO3 using MnO2 as a catalyst.
\[\ce{2KCI3 ->[MnO2] 2KCl + 3O2}\]
- Calculate the mass of KClO3 required to produce 6.72 litres of O2 at STP. [atomic masses of K = 39, Cl = 35.5, O = 16].
- Calculate the number of moles of oxygen present in the above volume and also the number of molecules.
- Calculate the volume occupied by 0.01 mole of CO2 at STP.
Solve the following:
What volume of oxygen is required to burn completely 90 dm3 of butane under similar conditions of temperature and pressure?
\[\ce{2C4H10 + 13O2 -> 8CO2 + 10H2O}\]
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)
Give two tests of the following:
Water vapour
The reaction between 15 g of marble and nitric acid is given by the following equation:
\[\ce{CaCO3 + 2HNO3 -> Ca(NO3)2 + H2O + CO2}\]
Calculate the mass of anhydrous calcium nitrate formed.
Nitrogen and hydrogen react to form ammonia.
\[\ce{N2_{(g)} + 3H2_{(g)}-> 2NH3_{(g)}}\]
If 1000g H2 reacts with 2000g of N2
Will any of the two reactants remain unreacted? If yes, which one and what will be its mass?
