Chemistry
Solid ammonium dichromate decomposes as under:
(NH₄)₂Cr₂O₇ ⟶ N₂ + Cr₂O₃ + 4H₂O
If 63 g of ammonium dichromate decomposes. Calculate
(a) the quantity in moles of (NH₄)₂Cr₂O₇
(b) the quantity in moles of nitrogen formed.
(c) the volume of N₂ evolved at S.T.P.
(d) the loss of mass
(iv) the mass of chromium (III) formed at the same time.
Related Questions
Find the percentage of
(a) oxygen in magnesium nitrate crystals [Mg(NO3)2.6H2O].
(b) boron in Na2B4O7.10H2O. H=1,B=11,O=16,Na=23.
(c) phosphorus in the fertilizer superphosphate Ca(H2PO4)2
What mass of copper hydroxide is precipitated by using 200 g of sodium hydroxide?
2NaOH + CuSO4 ⟶ Na2SO4 + Cu(OH)2 ↓
[Cu = 64, Na = 23, S = 32, H = 1]
Hydrogen sulphide gas burns in oxygen to yield 12.8 g of sulphur dioxide gas as under:
2H2S + 3O2 ⟶ 2H2O + 2SO2
Calculate the volume of hydrogen sulphide at S.T.P. Also, calculate the volume of oxygen required at S.T.P. which will complete the combustion of hydrogen sulphide determined in (litres).