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21 Cards in this Set
- Front
- Back
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Oxides are chemical compounds formed when an element reacts with Oxygen.
2Mg(s) + O₂(g) → 2MgO(s) |
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What Is Neutralisation? Write the word equation. |
The reaction between an acid and a base to produce a new compound that neither has acidic or basic properties.
Acid + Base → Salt + Water |
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Explain the difference between basic, acidic and amphoteric oxides. |
Basic oxides dissolves and reacts with a strong acid, where acidic oxides react with a strong base and an amphoteric oxide will react with both strong acids and strong bases and exhibits properties of both acidic and basic oxides. |
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Complete the following sentences: 1.Most Metal Oxides are... 2.Most Non-Metal Oxides are... 3.Most Semi-Metal Oxides are.. 4.Some oxides are ... 5.Some oxides have both... |
1.Basic Oxides 2.Acidic Oxides 3.Amphoteric 4. Neutral 5.Basic and acidic oxides properties. |
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What are the most common Industry generated oxides released into the atmosphere and write their chemical symbol? |
-Carbon Monoxide CO -Carbon Dioxide CO₂ -Sulfur Dioxide SO₂ -Oxides of Nitrogen NO(x) |
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List natural sources of Oxides of Carbon.
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-Animal and plant respiratory systems produce Carbon Dioxide -Bush Fires produce Carbon Monoxide and Carbon Dioxide (Carbon Monoxide is a result of incomplete combustion while Carbon Dioxide is the result of Complete combustion.) |
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List industrial sources of Oxides of Carbon. |
Combustion of fossil fuels such as kerosine, petrol and diesel oil releases large amounts of carbon oxides. Coal fired power plants release large amounts of Carbon Oxides as well.
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Increasing amounts of Carbon Dioxide in the atmosphere causes Global warming. Why doesn't Carbon Monoxide directly effect Global warming? |
Carbon Monoxide does not build up in the atmosphere over time as it is rapidly removed my soil organisms or by oxidation to carbon dioxide.
2CO + O₂ → 2CO₂ |
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State various sources of Oxides of Sulfur. |
Sulfur Dioxide is naturally released into the atmosphere by the eruption of volcanoes as well as the combustion of Organic matter in bush fires. Bacteria release H₂S(g) which then oxidises to form Sulfur dioxide. Sulfur Dioxide is Industrially created in the process of smelting ores of sulfur and the burning of coal, which contains small amounts (0.3%-1.0%) of minerals of of sulfur. Sulfur Dioxide also oxidises to form Sulfur Trioxide with the oxidants of Oxygen and Ozone. |
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Write a balanced equation for: a) the combustion of Minerals found in coal (FeS₂) b) the smelting of Chalcopyrite (CuFeS₂) c) the oxidation of SO₂ to SO₃ |
a)4FeS₂(s) + 11O₂(g) → 8SO₂(g) + 2Fe₂O₃(s) b)2CuFeS₂(s) + 5O₂(g) + 2SiO₂ → 2Cu + 4SO₂ + 2FeSiO₃ c) 2SO₂ + O₂ → 2SO₃ AND SO₂ + O₃ → SO₃ + O₂ |
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Identify the sources of Oxides of Nitrogen. |
Nitrogen Dioxide, Nitrogen Monoxide and Dinitrogen Oxide are the most common Oxides of Nitrogen and are known as the NOx gasses. These gasses are produced naturally by bacterial decomposition and lighting storms and are produced industrially from the emissions of motor vehicle engines and other tronsportation. |
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Explain the production of photochemical smog and how this has influenced the monitoring and restriction of emissions. |
When hydrocarbons and NOx gasses are in air containing moisture and ozone, sunlight reacts to form petrochemical smog. In 1952, 4000 people died in London from acidic smog and in the 1960's in cities such as Los Angeles and Tokyo, high measurements of petrochemical smog observed caused for the push for emission control. |
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Identify what procedures have been implemented for reducing levels of oxides of sulfur and nitrogen when burning coal. |
-Burning less coal by using energy efficient appliances and replacing fossil fuel energy production with renewable energy sources. -Burning coal containing less sulfur or switching to natural gas, which produces far less sulfur emission. |
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Identify what procedures have been implemented for reducing levels of oxides of sulfur and nitrogen other than when burning coal. |
-Collecting the sulfur from metal smelting and converting it to sulfuric acid. -Reducing acid emissions from smoke stacks by 'scrubbing' (the acidic gasses are passed through a slurry of base such as calcium oxide. SO₂(g) + CaO(aq) → CaSO₃(s) -Ensuring exhausts in motor vehicles pass though a catalytic converter (nitrogen oxides are converted back to nitrogen gas.) 2NO(g) + 2CO → N₂(g) + 2CO₂(g) |
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What is the typical pH of natural water? (Due to CO₂ dissolved in water) Write the chemical formula for how this water is made. |
6.0-6.5
CO₂(g) + H₂O(l) → H₂CO₃(aq) |
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Acid rain is formed by acidic oxides reacting with water. Write the equation for oxides and acids of both Nitrogen and Sulfur reacting with water. |
-SO₂ + H₂O → H₂SO₃ -SO₃ + H₂O → H₂SO₄ -2H₂SO₃ + O₂ → 2H₂SO₄ -2NO₂ + H₂O → H₂NO₂ + H₂NO₃ |
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How does acid rain affect man-made structures and statues? |
Acid rain causes marble and limestone statues and building to fade and erode. This is because the calcium carbonate is attacked by the sulfuric acid in the acid rain CaCO₃(s) + H₂SO₄(aq) → CaSO₄(aq) + H₂O(l) + CO₂(g) It also attacks iron and steel structures. It is oxidised by the Hydrogen ions in the acid and becomes chemically weathered. Fe(s) + H₂SO₄(aq) → FeSO₄(aq) + H₂(g) |
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How does acid rain affect the natural environment? |
Acid rain dissolves and take away mineral nutrients for plants in the soil such as calcium, magnesium and potassium. Metals such as aluminium that are normally insoluble can dissolve in the acid and release toxic metal ions into the soil, which is absorbed by the plants. Acid rain also causes lakes to significantly lower in pH. If the pH lowers too much, then it can kill marine life or cause marine life to loose the ability to reproduce. Fish eggs will not survive with a pH lower that 5.5 and adult fish will die if the acidity reaches below a pH of 5 as they can't extract sufficient calcium from the water for maintaining their skeleton. |
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List the requirements and characteristics of a chemical equilibrium. |
-The system is closed -The observable and measurable properties of the system are constant -The concentration of the products and reactants are constant once at equilibrium -The rate of the forward reaction equals the rate of backward reaction, thus the system is dynamic |
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Recall Le Chatelier's principle and identify the factors that cause a disturbance. |
'If a principle is at equilibrium and a change is made that disturbs the equilibrium, the the system responds in such a way as to counteract the change and eventually a new equilibrium is established'. The factors that may cause a disturbance are temperature, concentration or gas pressure. |
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The relationship between the number of moles (n) of a gas and the volume (V) is... |
n=V/Vm |
