Advertisements
Advertisements
Question
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]
Solution
\[\ce{2NaOH + CuSO4 -> Na2SO4 + Cu(OH)2 ↓}\]
Molecular mass of Cu(OH)2 = 64 + 16(2) + 1(2) = 98
Molecular mass of NaOH = 2(23 + 16 + 1) = 80
∴ 80 g sodium hydroxide forms = 98 g of Cu(OH)2
∴ 200 g sodium hydroxide will from = `(98 xx 200)/80`
= 245 g of Cu(OH)2
APPEARS IN
RELATED QUESTIONS
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.
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.
The ratio between the number of molecules in 2g of hydrogen and 32 g of oxygen is
[Given that H=1,O=16]
200 cm3 of hydrogen and 150 cm3 of oxygen are mixed and ignited, as per the following reaction,
\[\ce{2H2 + O2 → 2H2O}\]
What volume of oxygen remains unreacted?
The reaction between the red lead and hydrochloric acid is given below:
\[\ce{Pb3O4 + 8HCl -> 3PbCl2 + 4H2O + Cl2}\]
Calculate the volume of the chlorine evolved at S.T.P.
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:
\[\ce{3CuO + 2NH3 → 3Cu + 3H2O + N2}\]
66g of ammonium sulphate is produced by the action of ammonia on sulphuric acid. Write a balanced equation and calculate the volume of the gas used at STP.
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.
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.
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.
