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sulphur mixed with hydrogen sulphide what is result.
Nothing will happen if sulfur is mixed with hydrogen sulphide, but if sulfur is mixed with Na2S and heated we'll have according to the equation nS + Na2S = Na2S(n+1)...
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AT WHAT TEMPERATURE DOES THE ACTIVATED CHARCOAL ABSORB SULPHUR FROM SULPHUR-DIOXIDE
At the temperature of sulphur dioxide decomposition, i.e. over 4300 K.
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solid zinc metal reacts with sulfuric acid to form hydrogen gas and aqueous solution of zinc sulfate
Zn + H2SO4 → ZnSO4 + H2
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lead metal is obtained from lead sulphide through the following rection: 2PbS + 2C + 3O-2Pb + 2CO+2SO calculate mass oxygen is needed tu produce 500g of lead metal
Molar mass of Pb= 207.2g500/207.2= 2.413Mole ratio Pb:O2= 2:3Molar mass of O2= 31.998= 31.998×2.413×3/2= 115.823g
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4gm of a divalent metal reacts with chlorine to produce 11.1gm of its metal chloride. Calculate equivalent weight of the metal.
Calculate the atomic mass of the metal. 9. ... reacts with one-volume of chlorine to give two-volume hydrogen chloride gas. ... Equivalent weight of an element is 32.5. ... 4gm...
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What is the oxidation number and the correct formula and working outs for these; 1. Carbon in Sodium Carbonate 2. Sulphur in Hydrogen Sulphide 3. Nitrogen in Potassium Nitrate
1)Na2CO3=2+x-6=0X=42)H2S=2+X=0X=-23)KNO3=1+X-6=0X=5
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The percentage composition of a compound is 79.9% copper and 20.1% sulphur. The mass of a sample of the compound is 160.0 g. What are the masses of the copper and sulphur in the sample?
m = mcompound * W m(Cu) = 160 g * 0.799 = 127.84 g M(S) = 160 g * 0.201 = 32.16 g.
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you are given a powdered mixture of sulphur,potassium nitrate and carbon.state briefly how could you separate and collect each constituent in solid or powdered form?
1. Dissolve the mixture in enough quantity of water – KNO3 will dissolve. 2. Filter the solution and evaporate filtrate carefully – you’ll get KNO3 solid. 3. Heat gentle dried mixture of C...
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Solid zinc metal reacts with sulfuric acid to form hydrogen gas and an aqueous solution of zinc (II) sulfate.
Zn_solid+H_2 SO_4→ZnSO_4+H_2↑ n_solid – solid zinc H_2 SO_4 – sulfuric acid ZnSO_4 – zinc (II) sulfate H_2↑ – hydrogen gas
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The heat of combustion of sulphur in excess air to produce sulphur(iv)oxide is -297KJmol^-1. Calculate the heat change if 6.4g of sulphur is completely burned in excess air.(S=32)
While combustion of 1 mol of sulfur 297kJ/mol is released.From a given mass we found actual number of moles: n=m/M.n=6.4/32=0.2 (moles).∆H=0.2×(-297)=-59.4 (kJ/mol).
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