Question

Chapter 1 – Some Basic Concepts of Chemistry
Q1) 1.6 g of a hydrocarbon on complete combustion gave 4.4 g of CO2 and 3.6 g of H2O.
Show that this data proves law of conservation of mass.
Q2) 2.16g of copper metal when treated with nitric acid followed by ignition of the nitrate
gave 2.7 g of CuO. In another experiment 1.15g of copper oxide upon reduction with
hydrogen gave 0.92 g of copper. Show that the above data illustrates the law of definite proportion.
Q3) 3.2 g of sulphur combines with 3.2 g of oxygen to form compound in one set of
conditions. In another set 0.8 g of sulphur combines with 1.2 g of oxygen to form another
compound. State the law illustrated by the chemical combination.
Q4) Cu gives two oxides. On heating 1 g of each in hydrogen they gave 0.888 g of 0.799 g of
the metal respectively. Show that these results agree with law of multiple proportions.
Q5) Which of the following weighs the most:
(i) 50g of Fe (ii) 5g atoms of nitrogen (iii) 1x1023 atoms of carbon?
Q6) Calculate the amount present in grams in:
(a) 0.75 g atoms of sulphur (b) 2.5 g atom of phosphorus.
Q7) Calculate the number of molecules present in 280 mL of oxygen at STP.
Q8) Calculate the no. of molecules in a drop of water weighing 0.05 g.
Q9) 3 g of H2 reacts with 24 g of O2 to form H2O.
(i) Which is the limiting agent?
(ii) Calculate the maximum amount of H2O that can be formed.
(iii) Calculate the amount of the reactant is left unreacted.
Q10) What mass of slaked lime would be required to decompose completely 4 g of NH4Cl
and what would be the mass of each product?

Answer 1

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