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Chemistry c5 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

Recall the formula of hydrochloric acid

A

HCl

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2
Q

Recall the formula of Ethanoic Acid

A

CH3COOH

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3
Q

Recall the formula of carbon dioxide

A

CO2

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4
Q

Recall the formula of Hydrogen

A

H2

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5
Q

Recall the formula of Water

A

H2O

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6
Q

Recall the formula of sodium chloride

A

NaCl

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7
Q

Recall the formula potassium chloride

A

KCl

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8
Q

Recall the formula of calcium carbonate

A

CaCO3

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9
Q

Recall the formula of sulfuric acid and nitric acid

A

H2SO4 and HNO3

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10
Q

Recall the formula of sodium hydroxide, potassium hydroxide and magnesium carbonate

A

NaOH, KOH, MgCO3

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11
Q

Recall the formula of Sodium Sulfate

A

Na2SO4

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12
Q

Recall the formulas of Potassium Sulfate, Magnesium Sulfate, Barium Sulfate

A

K2SO4
MgSO4
BaSO4

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13
Q

Recall the formulas of Lead(II) Nitrate and Lead iodide

A

Pb(NO3)2

Pbl2

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14
Q

Recall the formulas of potassium iodide and potassium nitrate

A

Kl

KNO3

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15
Q

Recall and use the relationship between molar mass, number of moles and mass

A

number of moles = mass ÷ molar mass

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16
Q

Recall that the relative atomic mass of an element…

A

IS the average mass of an atom of the element compared to the mass of 1/12th of an atom of carbon-12.

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17
Q

Calculate empirical formula of a compound

A

1) Write each elements symbol
2) write each mass in g
3) write each ar
4) find the number of moles
5) divide by the smallest number
6) check for whole numbers, write the formula

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18
Q

Convert volume in cm3 into dm3 or vice versa

A

Divide or multiply by a thousand

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19
Q

Recall and use the relationship between the amount in moles, concentration in mol/dm3 and volume in dm3

A

amount in moles = concentration × volume

concentration = amount in moles ÷ volume volume = amount in moles ÷ concentration.

20
Q

Interpret information on food packaging about guideline daily amounts (GDA)

A

Figuring out percentages and amounts refer to page 177 for more Information

21
Q

Interpret more complex food packaging information and its limitations

A

Sodium chloride- common salt
Sodium ions it contains are needed for transmitting nerve signals and muscular contraction.
All foods contain salt in varying amounts and most processed foods contain added salt.
Too much salt can cause health problems including high blood pressure, leading to an increased risk of heart disease. The GDA for an adult is 6g.
The percentage by mass of sodium in sodium chloride is 39.3%. However sodium ions can come from other sources in food, so this conversion may be inaccurate.

22
Q

Sketch a pH titration curve for the titration of an acid or an alkali.

A

Acid to an alkali( high to low)

Alkali to an acid (low to high)

23
Q

Explain the need for several consistent titre readings in titrations.

A

It is important that the titre is accurate, otherwise the calculated concentration will be wrong. A titration is repeated until several consistent titres are obtained. Any anomalous titres are ignored and the mean titre is obtained.

24
Q

Describe the difference in colour change during a titration using a single indicator, such as litmus or phenolphthalein, compared to a mixed indicator, such as universal.

A

Phenolphthalein is pink in alkaline solutions and colourless in acidic solutions.
Litmus is blue in alkaline solutions and red in acidic solutions.
Universal indicator- the several different indicators changes colour over a different range of pH values. Red in acids and purple in alkalis

25
Q

Explain why an acid-base titration should use a single indicator rather than a mixed indicator.

A

As it does not allow you to know the precise end point in a titration. Phenolphthalein gives a sudden colour change between pink and colourless at the end point.

26
Q

Describe an experimental method to measure the volume of gas produced in a reaction given appropriate details about the reaction.

A

A gas syringe is used. It usually measures volumes up to 100cm3. Gas syringes can be used to measure the volume of any gas. The syringe is connected to the reaction container by tubing. As the reaction occurs, glass fills the gas syringe and pushes the plunger out. Graduations on the side show the volume of gas contained in the gas syringe.

27
Q

Describe an experimental method to measure the mass of gas produced in a reaction given appropriate details about the reaction.

A

Gases can also be collected over water in an upturned measuring cylinder. This is filled with water, then turned upside down in a trough of water. Air pressure keeps the water inside the cylinder. A delivery tube is led from the reaction container and into the mouth of the measuring cylinder. As the reaction occurs, gas fills the measuring cylinder and pushes the water out. Graduations on the side show the volume of gas contained

28
Q

Calculate the volume of a known number of moles of gas given the molar gas volume of 24 dm3 at room temperature and pressure (rtp). Calculate the amount in moles of a volume of gas at rtp given the molar gas volume at rtp.

A

The reaction container with its containers is placed on the balance. As the reaction takes place, the gas escapes and the total mass of the container and its contents is placed on the balance. As the reaction takes place, the gas escapes and the total mass of the container and its contents go down. The difference in mass is due to the gas that has escaped.

29
Q

Sketch a graph to show how the volume of gas produced during the course of a reaction changes, given appropriate details about the reaction.

A

The line starts off steeply and eventually becomes horizontal. It’s gradient decreases as the reaction continues. This shows that the rate of reaction decreases as the reaction continues. It’s is fastest at the start, when the gradient is the greatest. The reaction has stopped when the line becomes horizontal.

30
Q

Recall that in a reversible reaction at equilibrium:

A

The rate of the forward reaction equals the rate of the backward reaction. The concentrations of the reactants and the products do not change. The position of equilibrium is related to the ratio of the concentration of the products to the concentration of the reactants.

31
Q

Explain why a reversible reaction may reach an equilibrium:

A

Importance of a closed system.initially rate of forward reaction decreases. Initially rate of backward reaction increases. Eventually rate of forward equals rate of backward reaction.

32
Q

Understand in simple qualitative terms factors that affect the position of equilibrium:

A

removing a product moves the position of equilibrium to the right or vice versa.adding extra reactant moves the position of equilibrium to the right or vice versa. increasing the temperature moves the position of equilibrium in the direction of the endothermic reaction or vice versa. increasing the pressure moves the position of equilibrium to the side with the least number of moles of gas molecules or vice versa.

33
Q

Understand that the reaction between sulfur dioxide and oxygen is reversible:
Describe the conditions used in the Contact Process:

A

sulfur dioxide + oxygen sulfur trioxide

2SO2(g) + O2(g) 2SO3(g)

34
Q

Describe the conditions used in the Contact process.

A

V2O5 catalyst, around 450°C and atmospheric pressure.

35
Q

Explain the conditions used in the Contact Process

A

increasing the temperature moves the position of equilibrium to the left and increases rate of reaction so a compromise temperature is used.addition of catalyst increases rate but does not change position of equilibrium even at low pressure, the position of equilibrium is already on right so expensive high pressure is not needed.

36
Q

Acid ionising in water.

A

An acid ionises in water to produce H+ ions. Understand that a strong acid completely ionises in water and a weak acid does not fully ionise and forms an equilibrium mixture.

37
Q

Explain why the pH of a weak acid is much higher than the pH of a strong acid of the same concentration.

A

Hydrochloric acid is completely ionised in water whereas ethanoic acid is only partially ionised in water. So for a given concentration of acid, the concentration of hydrogen ions is greater in hydrochloric acid that it is in ethanoic acid. This is why the pH of a strong acid is much lower that the pH of a weak acid at the same concentration.

38
Q

Explain the difference between acid strength and acid concentration:

A

acid strength (strong or weak) is a measure of the degree of ionisation of the acid. acid concentration is a measure of the number of moles of acid in one d

39
Q

Explain why ethanoic acid reacts slower than hydrochloric acid of the same concentration:

A

Ethanoic acid has a lower concentration of hydrogen ions. In ethanoic acid the hydrogen ions have a lower collision frequency with reactant particles.

40
Q

Explain why ethanoic acid is less conductive than hydrochloric acid of the same concentration:

A

lower concentration of hydrogen ions to carry the charge in ethanoic acid.

41
Q

Explain, in terms of collisions between ions, why most precipitation reactions are extremely fast.

A

The collision frequency between ions in solution is very large. There is a high chance that different ions will collide with each other and cause a reaction, so precipitation reactions are extremely fast. Precipitates form as soon as two suitable solutions are mixed together.

42
Q

Interpret experimental data about the testing of solutions using aqueous barium chloride and aqueous lead nitrate.

A

Barium ions and Sulfate ions will make a precipitate together. Barium Sulfate precipitate is the product.

43
Q

Construct word equations for simple precipitation reactions e.g. for the reaction between solutions of barium chloride and sodium sulfate (products not given).

A

Barium chloride+ sodium Sulfate —> sodium Sulfate + barium Sulfate

44
Q

Construct ionic equations, with state symbols, for simple precipitation reactions, given the formulae of the ions that react. Explain the concept of ‘spectator ions’

A

Ba2+ (aq)+ So2-4 (as)—> BaSO4(s)

Spectator ions don’t take part in the reaction but instead form the other product.

45
Q

Describe the stages involved in the preparation of a dry sample of an insoluble compound by precipitation given the names of the reactants

A

mix solutions of reactants, filtration, wash and dry residue

Chemistry c5 (1 decks)

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