Some Basic Concepts Flashcards

1
Q

Law of Conservation of mass

A

Matter can neither be created nor destroyed

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2
Q

Law of definite proportions

A

A given compound always contains exactly the same proportion of elements by weight

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3
Q

Law of Multiple Proportions

A

If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole numbers

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4
Q

Gay Lussac’s Law

A

When gases combine or are produced in a chemical reaction they do so in a simple ratio by volume, provided all gases are at same temperature and pressure

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5
Q

Avogadro’s Law

A

Equal volumes of all gases at the same temperature and pressure should contain equal number of molecules

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6
Q

Amount present in one mole

A

Avogadro Number - 6.022*(10^23)

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7
Q

Mass by mass percentage

A

(Mass of element / Mass of compound)*(100)

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7
Q

Finding molecular formula

A

Molar mass / Empirical formula = n
Putting n moles in empirical formula

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7
Q

Steps for calculating empirical formulas

A
  1. Take percentage as in grams
  2. Find moles of each element
  3. Simplify in simplest whole number ratio
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8
Q

Limiting reagent

A

Reactant, which gets consumed first, limits the amount of product formed

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9
Q

Mole Fraction

A

Ratio of number of moles of a particular component to the total number of moles in the solution
(Na / (Na + Nb))

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10
Q

Molarity

A

M =Number of moles of solute / (Volume of solution in Litres)

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11
Q

Formula for molarity (when two solutions)

A

M1V1 = M2V2

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12
Q

Molality

A

m = no. of moles of solute / mass of solvent in kg

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13
Q

If the density of methanol is 0.793 kg L–1, what is its volume needed for making 2.5
L of its 0.25 M solution?

A

Using, M1V1 = M2V2:
0.793/0.032 = 24.78M
24.78V1 = 0.25 * 2.5L
V1 = 25.22mL

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14
Q

Calculate the molarity of a solution of ethanol in water, in which the mole fraction of
ethanol is 0.040 (assume the density of water to be one).

A

2.314M

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23
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