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And it gives the conversion factor of 1 / 58.5. Now multiply 25 g with 1 /58.5, which is same as dividing 25 / 58.5. This tells us that there are 0.427 moles of NaCl in the solution. Now you can use these numbers in the equations: Molarity = moles of solute / litres of solution. Molarity = 0.427 / 2 = 0.214 M.
Mole can be defined as the amount of substance that contains the same number of entities (atoms, molecules, ions etc) as the number of atoms present in 12 g of the carbon − 12 isotope. Mole represents 6.022 × 10 23 particles ( A l s o c a l l e d A v o g a d r o n u m b e r N A )
Avagadro’s Number. The number of particles present in one mole of any substance is 6.022 X 10 23. This value is the Avogadro number. So 1 mole = 6.022 X 10 23 particles in number. So, the mass of one mole of a molecule or ion is equivalent to its relative atomic or molecular mass in grams. Avagadro number is named after the Amadeo Avagadros ...
View Solution. Calculate the mole fraction of Benzene in a solution containing 30% by mass in . (Cl = 35.5) View Solution.
The number of sodium atoms present = 1. The number of chlorine atoms present = 1. Mass of a sodium atom = 989770 amu. Mass of an oxygen atom = 45 amu. Therefore the molecular weight of H 2 O = (1x 99 amu) + (1 x 35.45 amu) = 58.44 amu. With the help of the above example, we can say that both molar mass and molecular mass are the same in their ...
Mole fraction refers to a unit of concentration. It is a formula in the field of physics that is unitless expression. Mole fraction is equal to the number of a component’s moles divided by the total number of a solution’s moles. Also, when analyzing the solutions chemist use mole formula to measure the concentration of components.
Q 1. Define mole fraction. A solution of sucrose in water is labelled as 20 % w/w. What would be the mole fraction of each component in the solution? View Solution. Q 2.
Hence, one mole of oxygen weighs 32 g. One mole of oxygen contains 6.023 ...
Calculate the work done during isothermal expansion of one mole of an ideal gas from 10 atm to 1 atm at 300 K.
The mass of 1 mole of it is 42 g. The molecular formula of the compound is: View Solution. Q3.
