Chemistry
Define the terms – (a) Relative atomic mass (b) Relative molecular mass. State why indirect methods are utilized to determine the absolute mass of an atom. Explain in brief the indirect method used.
Related Questions
Balance the following important equations :
NaHCO3 + H2SO4 ⟶ Na2SO4 + H2O + CO2
NaOH + H2SO4 ⟶ Na2SO4 + H2O
Pb(NO3)2 + NaCl ⟶ NaNO3 + PbCl2
FeSO4 + NaOH ⟶ Na2SO4 + Fe(OH)2
FeCl3 + NaOH ⟶ NaCl + Fe(OH)3
CuSO4 + NaOH ⟶ Na2SO4 + Cu(OH)2
FeCl3 + NH4OH ⟶ NH4Cl + Fe(OH)3
ZnO + NaOH ⟶ Na2ZnO2 + H2O
Pb(OH)2 + NaOH ⟶ Na2PbO2 + H2O
Al2O3.2H2O + NaOH ⟶ NaAlO2 + H2O
NaAlO2 + H2O ⟶ NaOH + Al(OH)3
Al(OH)3 ⟶ Al2O3 + H2O
ZnS + O2 ⟶ ZnO + SO2
Fe2O3 + Al ⟶ Al2O3 + Fe
Al + Cl2 ⟶ AlCl3
NaCl + H2SO4 ⟶ Na2SO4 + HCl
Fe + HCl ⟶ FeCl2 + H2
Na2CO3 + HCl ⟶ NaCl + H2O + CO2
Pb(NO3)2 + HCl ⟶ PbCl2 + HNO3
AgCl + NH4OH ⟶ Ag(NH3)2Cl + H2O
MnO2 + HCl ⟶ MnCl2 + H2O + Cl2
Pb3O4 + HCl ⟶ PbCl2 + H2O + Cl2
KMnO4 + HCl ⟶ KCl + MnCl2 + H2O + Cl2
K2Cr2O7 + HCl ⟶ KCl + CrCl3 + H2O + Cl2
NH4Cl + Ca(OH)2 ⟶ CaCl2 + H2O + NH3
(NH4)2SO4 + NaOH ⟶ Na2SO4 + H2O + NH3
Mg3N2 + H2O ⟶ Mg(OH)2 + NH3
AlN + H2O ⟶ Al(OH)3 + NH3
NH3 + O2 ⟶ N2 + H2O [burning of NH3]
NH3 + O2 ⟶ NO + H2O [Catalytic oxidation of NH3]
NH4OH + H2SO4 ⟶ (NH4)2SO4 + H2O
NH3 + CuO ⟶ Cu + H2O + N2
NH3 + Cl2 ⟶ HCl + NCl3 [nitrogen trichloride]
HNO3 ⟶ H2O + NO2 + O2
Ca(HCO3)2 + HNO3 ⟶ Ca(NO3)2 + H2O + CO2
C + HNO3 [conc.] ⟶ CO2 + H2O + NO2
S + HNO3 [conc.] ⟶ H2SO4 + H2O + NO2
Cu + HNO3 [conc.] ⟶ Cu(NO3)2 + H2O + NO2
C + H2SO4 [conc.] ⟶ CO2 + H2O + SO2
S + H2SO4 [conc.] ⟶ SO2 + H2O
Cu + H2SO4 [conc.] ⟶ CuSO4 + H2O + SO2
Give balanced equations for (1) & (2) by partial equation method, [steps are given below]
- Reaction of excess ammonia with chlorine – Ammonia as a reducing agent
(a) Ammonia first reacts with chlorine to give hydrogen chloride and nitrogen.
(b) Hydrogen chloride then further reacts with excess ammonia to give ammonium chloride. - Oxidation of Lead [II] Sulphide by Ozone
(a) Ozone first decomposes to give molecular oxygen & nascent oxygen.
(b) Nascent oxygen then oxidizes lead [II] sulphide to lead [II] sulphate.
- Reaction of excess ammonia with chlorine – Ammonia as a reducing agent
Calculate relative molecular mass of
(a) ZnCO3
(b) CaSO4[Zn = 65, S = 32, O = 16, Ca = 40, C = 12]
Calculate the percentage composition of
(a) calcium chloride
(b) calcium nitrate[Ca = 40 , Cl = 35.5 , N = 14 , O = 16]