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Chemistry > Physical - Amount of Substance > Flashcards

Physical - Amount of Substance Flashcards

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1
Q

What is the rule with significant figures?

A

With significant figures, your final answer should be given to the same number of significant figures as the least number of significant numbers used in the data given.

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2
Q

What is the rule with decimal places?

A

With decimal places, we round our answer to the data with the fewest number of decimal places.

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3
Q

What are SI Units?

A
  • International system of units.
  • There are 7 base units from which all other units are derived.
  • There are 20 prefixes which show multiples or
    fractions of the base quantity.
  • The base units are derived from invariable constants in nature, e.g. the speed of light.
  • Adopted by all countries except the US, Liberia and Myanmar.
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4
Q

What is the relative atomic mass?

A

The relative atomic mass Ar is the weighted average mass of an atom of an element, taking into account its naturally occurring isotopes, relative to 1/12th the relative atomic mass of an atom of carbon-12.

average mass of one atom of an element / (mass of one atom of carbon-12 x 1/12)

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5
Q

What is the relative molecular mass?

A

The relative molecular mass Mr of a molecule is the mass of that molecule compared to 1/12 the relative atomic mass of an atom of carbon-12.

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6
Q

What is the Avogadro constant?

A

The Avogadro constant or Avogadro number is the number of atoms in 12g of carbon-12.

6.022x10^23

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7
Q

What is the mole?

A

The amount of substance that contains 6.022x10^23 particles is called a mole.

The relative atomic mass of any element in grams contains one mole of atoms. The relative molecular mass (or relative formula mass) of a substance in grams contains one mole of entities. You can also have a mole of ions or electrons.

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8
Q

How do you work out the number of moles?

A

mass / Mr

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9
Q

What is the relative formula mass?

A

The relative molecular mass for ionic compounds.

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10
Q

Why is the volume of a given mass of any gas not fixed?

A

It changes with pressure and temperature. However, there are a number of simple relationships for a given mass of gas that connect the pressure, temperature, and volume of a gas.

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11
Q

What is Boyle’s law?

A

The product of pressure multiplied by the volume of a gas in an enclosed container remains the same if either the pressure or volume changes and the temperature remains constant.

Pressure and volume are inversely proportional.

pressure x volume = constant

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12
Q

What is Charles’ law?

A

The volume is directly proportional to the temperature as long as the pressure remains constant.

volume / temperature = constant

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13
Q

What is Gay-Lussac’s law? (the constant volume law)

A

The pressure of a gas varies directly with the absolute temperature of the gas when volume remains constant.

pressure / temperature = constant

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14
Q

What equation does combining these relationships give?

A

(pressure x volume) / temperature = constant for a fixed mass of gas

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15
Q

What is the ideal gas equation?

A

In one mole of gas, the constant is given the symbol R and is called the gas constant. For n moles of gas:

pressure P (Pa) x volume V (m3) = number of moles n x gas constant R (J K-1 mol-1) x temperature T (K)

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16
Q

What is the value of R?

A

8.31 JK-1 mol-1

17
Q

Why is it called the ideal gas equation?

A

No gases obey it exactly, but at room temperature and pressure it hold quite well for many gases. It is often useful to imagine a gas which obeys the equation perfectly - an ideal gas.

18
Q

What is the empirical formula?

A

The empirical formula is the formula that represents the simplest whole number ratio of the atoms of each element present in a compound.

19
Q

How do you find the empirical formula?

A
  1. Find the masses of each of the elements present in a compound (by experiment).
  2. Work out the number of moles of atoms of each element.
    number of moles = mass of element / mass of 1 mol of element
  3. Convert the number of moles of each element into a whole number ratio by dividing each answer by the smallest answer.
20
Q

What is the molecular formula?

A

The molecular formula gives the actual number of atoms of each element in one molecule of the compound (it applies only to substances that exist as molecules).

21
Q

How do you find the molecular formula?

A

To find the number of units of the empirical formula in the molecular formula, divide the relative molecular mass by the relative mass of the empirical formula.

22
Q

What is an ideal gas?

A

In an ideal gas:

  • collisions are perfectly elastic
  • no intermolecular attractive forces (i.e. all internal energy = kinetic energy)
  • therefore does not condense into a liquid when cooled
23
Q

What is molar volume?

A

The volume occupied by 1 mole of a gaseous substance is called its molar volume. Molar volume can be calculated from the density of the gas and its formula mass, Mr. Since volume depends on both temperature and pressure, molar volume is generally measured at “room temperature and pressure”, which is about 20 degrees Celsius and 1 atmosphere.

24
Q

What is the molar volume equation?

A

molar volume = mass of 1 mole / density at rtp

25
Q

What is the molar volume of any gas at rtp?

A

24dm3

26
Q

What is combustion analysis?

A

Organic compounds are based on carbon and hydrogen. One method of finding empirical formulae of new compounds is called combustion analysis. It is used routinely in the pharmaceutical industry. It involves burning the unknown compound in excess oxygen and measuring the amounts of water, carbon dioxide, and other oxides that are produced. The gases are carried through the instrument by a stream of helium.

27
Q

What is stoichiometry?

A

The ratio in which the reactants react and the products are produced, in simple whole numbers, is called the stoichiometry of the reaction. You can build up a stoichiometric relationship from experimental data by working out the number of moles that react together. This leads to a balanced symbol equation.

28
Q

What are spectator ions?

A

ions that do not take part in the reaction

29
Q

What is atom economy?

A

mass of desired product / total mass of reactants

30
Q

What is the difference between atom economy and the yield?

A

The atom economy tells us in theory how many atoms must be wasted in a reaction.

The yield tells us about the practical efficiency of the process.

31
Q

How may reactants be lost?

A
  • the practical process of obtaining a product (not all product is recovered)
  • as a result of reactions that do not go to completion
  • reaction impurities
  • a side reaction occurs
  • inaccuracy in measurement
32
Q

What is the percentage yield?

A

(actual yield / theoretical yield) x 100

33
Q

Why is it desirable to have a high atom economy?

A

In industrial chemical processes, it is desirable to have a high atom economy for a reaction. This means there is little or no waste product, only the desired product. Therefore it means the process is more economically viable for industrial scale manufacture. Having a high atom economy is also beneficial for the environment as it uses less natural resources and therefore often uses less energy.

34
Q

What are the steps for titration?

A
  1. Rinse out pipette with the solution you are about to use.
  2. Fill the pipette with the unknown solution.
  3. Initially take more than required.
  4. Carefully release the solution until the bottom of the meniscus is touching the line.
  5. Transfer to a clean conical flask.
  6. The pipette is calibrated, so touch the pipette to liquid in flask to remove all solution (not blow!).
  7. The amount in the pipette is called the aliquot (usually 25cm3).
  8. Fill Burette at eye level with your known solution.
  9. Check the tap is closed! Fill using a funnel, tilted slightly. Add 2 or 3 drops of indicator.
  10. Carry out a titration (rough).
  11. Remember to swirl the flask continuously.
  12. Stop when permanent colour change is observed (the end point).
  13. For the accurate run, 5cm3 before the end, start adding solution dropwise. Repeat until successive titres are within 0.1 cm3.
  14. Titres that are within 0.1cm3 are called concordant.

Chemistry (38 decks)

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