Some Basic Conc...

According to Avogadro's hypothesis, equal volumes of gases under the same conditions of temperature and pressure will contain:

'Equal volumes of all gases at the same temperature and pressure contain equal number of molecules'. This law is called as

Thermal electricity is generated from:

A sample of calcium carbonate $$(CaCO_{3})$$ has the following percentage composition: $$Ca = 40\%; \ C = 12\%; \ O = 48\%$$.
If the law of constant proportions is true, then the weight of calcium in $$4 g$$ of a sample of calcium carbonate from another source will be:

An impure sample of silver $$(1.5\ g)$$ is heated with $$S$$ to form $$0.124\ g$$ of $$Ag_2S$$. What was the per cent yield of $$Ag_2S$$?

0.46 g of an organic compound  was analysed. The increase in mass of $$ CaCl_2$$ U-Tube  was 0.54 g and potash bulb was 0.88 g. The percentage composition  of the compound is:

Which scientist discovered that the same amount of space was occupied by equal numbers of molecules of gases, irrespective of whether it was hydrogen or chlorine or fluorine?

Read the passage given below and answer the question:
Chemical reactions involve the interaction of atoms and molecules. A large number of atoms/molecules (approximately $$6.023 \times 10^{23}$$) are present in few grams of any chemical compound varying with their atomic/molecular masses. To handle such large numbers conveniently, the mole concept was introduced. This concept has implications in diverse areas such as analytical chemistry,  biochemistry, electrochemistry, and radiochemistry. the following example illustrates a typical case, involving chemical/electrochemical reaction, which requires a clear understanding of the mole concept.
A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: Na = 23, Hg = 200; 1 faraday =96500 coulombs). 
If the cathode is a Hg electrode, the maximum weight (g) of amalgam formed from this solution is:

The number of atoms in 67.2 L of $${ NH }_{ 3 }$$(g) at STP is:

A $$10.0g$$ a sample of a mixture of calcium chloride and sodium chloride is treated with $$Na_2CO_3$$ to precipitate the calcium as calcium carbonate. This $$CaCO_3$$ is heated to convert all the calcium to $$CaO$$ and the final mass of $$CaO$$ is $$1.62gms$$. The $$\%$$ by mass of $$CaCl_2$$ in the original mixture is :