2.56 f of suphur in 100 g of `CS_(2)` has depression in freezing point of 0.010^(@) K_(f)=0.1^(@)` (molal)^(-1)`. Hence atomicity of sulphurin the solution is

2.56 g of suphur in 100 g of CS_(2) has depression in freezing point of 0.010^(@)C , K_(f)=0.1^(@)C (molal)^(-1) . Hence atomicity of sulphur in the solution is

2.56 g of sulphur in 100 g of CS_2 has depression in freezing point of 0.010^@ . K_(f)=0.1^(@) kg (mol)^(-1) . Hence atomicity of sulphur in the solution is

2.56g of sulfur in 100 g of CS_(2) of has depression in freez point of 0.01^(@)C.K_(f)=0.1^(@) mol al^(-1) . Hence, he atomicity of sulfur is CS_(2) is

2.56g of sulfur in 100 g of CS_(2) of has depression in freez point of 0.01^(@)C.K_(f)=0.1^(@) mol al^(-1) . Hence, he atomicity of sulfur is CS_(2) is

2.56g of sulfur in 100 g of CS_(2) of has depression in freez point of 0.01^(@)C.K_(f)=0.1^(@) mol al^(-1) . Hence, he atomicity of sulfur is CS_(2) is

20 g of a binary electrolyte(mol.wt.= 100 )are dissolved in 500 g of water.The freezing point of the solution is -0.74^(@)CK_(f)=1.86K "molality"^(-1) .the degree of ionization of the electrolyte is

20 g of a binary electrolyte(mol.wt.= 100 )are dissolved in 500 g of water.The freezing point of the solution is -0.74^(@)CK_(f)=1.86K "molality"^(-1) .the degree of ionization of the electrolyte is

When 2.56 g of sulphur was dissolved in 100 g of CS_(2) , the freezing point lowered by 0.383 K. Calculate the formula of sulphur (S_(x)) . ( K_(f) for CS_(2) = 3.83 K kg mol^(-1) , Atomic mass of sulphur = 32g mol^(-1) ]