Identification of Common Gases (AQA GCSE Chemistry)

Limestone is used as a building material even though it is eroded by acid rain.

Limestone contains the compound calcium carbonate which reacts with hydrochloric acid as shown.

CaCO₃ (s) + 2HCl (aq) → CaCl₂ (aq) + H₂O (l) + CO₂ (g)

Describe a test to show that CO₂ is produced in the reaction.

Gases expelled from the exhausts of vehicles produce sulfuric acid and nitric acid.

• A student investigated the reaction of both acids with limestone.

• Only the type of acid was changed, all other variables in the investigation were kept the same. 

• The student measured the volume of CO₂ gas produced every minute for a total of 10 minutes. 

• The first reaction studied was between dilute sulfuric acid and a cube of calcium carbonate.

• The student then repeated the experiment using dilute nitric acid. 

The results are shown in Figure 1.

Figure 1

State three variables that must be kept the same for this investigation.

Different results were obtained for reacting calcium carbonate with sulfuric acid than with nitric acid.

The equations for both reactions are shown below.

CaCO₃ (s) + H₂SO₄ (aq) → CaSO₄ (s) + H₂O (l) + CO₂ (g)

CaCO₃ (s) + 2HNO₃ (aq) → Ca(NO₃)₂ (aq) + H₂O (l) + CO₂ (g)

Describe how the results for sulfuric acid are different and explain this difference with reference to the symbol equations.

During the electrolysis of brine, chlorine gas forms at one electrode.

2Cl^- (aq) Cl₂ (g) + 2e^-

Which test would be most appropriate to confirm that chlorine gas was produced?

Which is the correct method for testing for hydrogen gas?

A fungicide suitable for crops contains copper sulfate, CuSO₄, and ammonium carbonate, (NH₄)₂CO₃.         

A student tested a sample of the fungicide.

Hydrochloric acid was added and a gas was produced that turned limewater milky.

Complete the sentences. 

The gas produced was _________________________ which shows that _________________________ ions are in the mixture. 

The formula for the ion is: ________

Describe a method for testing the carbon dioxide gas produced from the reaction of ammonium carbonate, (NH₄)₂CO₃ and hydrochloric acid, HCl.

You may use a diagram.

Next, sodium hydroxide solution was added to a sample of the fungicide.

A gas was produced indicating that ammonia was produced.

Ammonia can react with chlorine gas to form hydrochloric acid and then ammonium chloride, a white powder. These are not the desirable products.

Describe how the gas in the reaction vessel could be tested in order to check for the presence of chlorine. 

Complete the sentence. 

The gas in the vessel could be tested using damp ____________________ which turns _____________________ if chlorine gas is present.

Chlorine gas also has a distinctive smell, like the smell of swimming pools and bleach.

Why should this not be used as a test to identify the gas?

Methane, CH₄ contains the elements carbon and hydrogen only.

A student wanted to find out which new substances are produced when methane is burned.

The student set up the apparatus shown below.

Which gas in the air reacts with methane when it burns?

Name the liquid collected.

Name the gas which turns limewater milky.

When methane burns an exothermic reaction takes place.

What is meant by an exothermic reaction?

Hydrogen peroxide, H₂O₂, is often used as a bleach. It decomposes forming water and oxygen.

Write the balanced chemical equation for the decomposition of hydrogen peroxide.

Give a test for oxygen. 

Test: _________________________

 Result of test: _________________________

Describe the test for hydrogen. 

Test: _________________________ 

Result of test: _________________________

Two experiments were carried out to test if the mass of a manganese dioxide catalyst, MnO₂, affected the rate at which the hydrogen peroxide decomposed.

Complete Figure 1 to show how you could measure the volume of oxygen formed during the decomposition.

Figure 1

The same volume and concentration of hydrogen peroxide solution was used for both experiments.

What two other factors must be kept the same to make it a fair test?

Which is not true about the test for carbon dioxide gas?

The electrolysis of fresh water produces hydrogen gas and oxygen gas.

The electrolysis of salt water (brine) produces hydrogen gas and chlorine, and leaves a solution of sodium hydroxide.

Which test would not help to identify a sample as being fresh water or salt water?

Sodium hydrogencarbonate, NaHCO₃, is an alkali that undergoes a neutralisation reaction with sulfuric acid, H₂SO₄.

Write the balanced symbol equation for this reaction.

One of the active ingredients in baking powder is sodium hydrogencarbonate. It also contains an acid.

When water is added to baking powder, carbon dioxide is released.

Outline how you could test to confirm the presence of carbon dioxide.

Sodium hydrogencarbonate is also used in indigestion tablets.

Indigestion is caused by excess hydrochloric acid in the stomach.

A side effect of taking indigestion tablets can be a build up of gas in the stomach which causes stomach pain and bloating

Explain why.

A student made a standard solution of 0.5 mol/dm³ sodium hydrogencarbonate.

What mass of sodium hydrogencarbonate needs to be added to 250 cm³ of distilled water to obtain this concentration?

Relative atomic masses (A_r):  H = 1;  C = 12,  O = 16,  Na = 23

A student investigated photosynthesis of algae by placing some algae in water with a light shining onto the algae.

The water contained a dissolved gas necessary for photosynthesis to occur.

Name the dissolved gas.

As photosynthesis occurred, gas bubbles were seen and the resulting gas was collected.

Describe a test that could be performed to identify the gas collected.

Give the results of the test.

The student increased the light intensity which was shining on the beaker containing algae and water.

How would the observations the student would make be different after increasing the light intensity?

Explain your answer.

A student investigated how the volume of gases produced changed with time during the electrolysis of sodium chloride solution.

Figure 1 shows the equipment the student used.

Figure 1

Why is hydrogen gas, not sodium, collected at the cathode?

Chlorine gas is collected at the anode.

Write the half equation for the reaction at the anode.

Describe a test for chlorine gas.

Give the result of the test if chlorine is present.

The student recorded the results shown in Table 1.

Table 1

The volume of one mole of any gas at room temperature and pressure is 24.0 dm³_.

The number of moles of hydrogen and chlorine gas produced at each electrode is the same.

Suggest why the volume of gas collected at each electrode is not the same.

Assume no gas has escaped from the apparatus.

Calculate the amount in moles of hydrogen collected after 16 minutes.

Use Table 1.

Give your answer to two significant figure.

A student investigated how the rate of reaction between magnesium and hydrochloric acid changed with temperature, shown in Figure 1.

The student measured the time for the magnesium to stop reacting.

Figure 1

The equation for the reaction is:

Mg(s) + 2HCl(aq)    →      MgCl₂(aq)  +  H₂(g)

Describe a test for hydrogen gas.

Give the result of the test if hydrogen is present and given the balanced symbol equation for the reaction that occurs if hydrogen is present.

State and explain what would happen to the rate of reaction between magnesium and hydrochloric acid as the temperature increased.

2.0 g of magnesium reacted with 25.0 cm³ of 1.0 mol/dm³ hydrochloric acid.

Calculate the volume of hydrogen gas that you would expect to be produced in this reaction.

Give your answer in dm³.

Assume the reaction occurs at room temperature and pressure.

The student repeated the experiment but used a white powder, compound X, instead of magnesium.

A gas was produced during the reaction with hydrochloric acid. When the gas was bubbled through turned limewater, it turned cloudy.

The student carried out a flame test on compound X and a lilac flame was produced.

Give the formula of compound X.