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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?

Md Ariful Islam

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Md Ariful Islam

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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 S. Melting point of sulfur is about 1130C – you will separate sulfur in liquid state (cool it and get solid S). Carbon stays.
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1) Enzymes are in which state of matter (solid, liquid, gas)? 2) Can enzymes be converted into solid state? 3) Do enzymes function if they are converted into solid state?

Solution1.Enzymes are generally in fluid form to enable them carry out metabolic functions2. Enzymes can be converted to solid state3. Converting leads to denaturing of the enzymes, the active side...

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What volume (in mL) of 0.50 M potassium nitrate contains 0.021 mol of potassium nitrate?

M=mol/volume Volume=mol/MV= 0.021÷0.5 = 0.042 LVolume in Ml = 0.042×1000Ans= 42mL

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You are to make 10.0 L of 1.20 M Potassium nitrate solution. What molarity would the potassium nitrate solution need to be if you were to use only 2.50 L of it?

Molarity needed for Potassium Nitrate Solution ;=4.8M

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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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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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A 0.4230 g sample of impure sodium nitrate was heated, converting all the sodium nitrate to .1235 g of sodium nitrate and oxygen gas. Determine the percent of sodium nitrate in the original sample.

Answer:2HNO3 = 2HNO2 + O2m= 85 x 0.1235 / 69= 0.1521W%= 0.1521 / 0.4230 = 36%

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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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Powdered zinc metal reacts with sulphur (S8) when heated to produce zinc sulphide.

equation of reaction: Zn + S=ZnS

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A volume of 20litres of HCL was completely decomposed to its constituent elements hydrogen and chlorine what are the volumes of the constituent elements

Balanced chemical reaction ,2HCl -----> H2 + Cl2From balanced chemical reaction, 2 L of HCl gives 1 L of each product Hence volume produced of H2 = [10] Lvolume...

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