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Paper 1 2019

Last updated 5 months ago
57 questions
1
In a hydrogen-oxygen fuel cell, hydrogen and oxygen react at the electrodes.
The overall reaction occurring in this fuel cell is a reaction of hydrogen with oxygen. Write the balanced equation for this reaction.
(2 marks)

______ H2​+O2​⟶______ H2​O
Other Answer Choices:
2
1
3
1
The electrodes of a fuel cell are in contact with water and air. The electrodes are made of platinum rather than iron.
State why iron is not a suitable metal for the electrodes of the cell.
(1 mark)
(i) Iron would react (with water / oxygen) / ____________
Other Answer Choices:
corrode
dissolve
explode
1
Platinum acts as a catalyst. State, in terms of its position in the periodic table, why you would expect platinum to act as a catalyst.
(1 mark)
Platinum is in group a _____________________
Other Answer Choices:
alkali metal
transition metal
noble gas
2

(c) Some metal objects are electroplated.
State two reasons for electroplating a metal object.

2

(c) Some metal objects are electroplated.
State two reasons for electroplating a metal object.

  • To improve appearance
  • for decoration
  • to prevent corrosion
  • to make it harder
  • To make it more gansta
  • This is a valid reason
  • This is not a valid reason
1

Periodic table


Using the letters A, E, G, J, X and Z, give the letters of the two elements that are non-metals.

1

Periodic table


Give the letters of two elements in period 2. (NOTE THERE ARE IN FACT 3)

1

Periodic table

Give the letter of an element that normally forms an ion with a charge of +1 (GIVE BOTH)
.

2
Element E has an atomic number of 5. In a sample of E there are two isotopes. One isotope has a mass number of 10 and the other isotope has a mass number of 11.
Explain, in terms of subatomic particles, what is meant by the term isotopes
Isotopes are atoms with the same number of ____________ but different numbers of _____________
Other Answer Choices:
protons
neutrons
1


All atoms of element E in this sample contain

1

Element X has an atomic number of 18. State the electronic configuration of an atom of element X.

3
In an experiment, 3.5 g of element A reacted with 4.0 g of element G to form a compound. Calculate the empirical formula of this compound.
(relative atomic masses: A = 7, G = 16)
You must show your working.
Moles of A = mass / RAM = 3.5 / 7 = ________
Moles of G = mass / RAM = 4 / 16 = _________
Divide by smallest value:
A = 0.5 / 0.25 = ______
G = 0.25 / 0.25 = ______
Empirical formulae = ________
Other Answer Choices:
2
0.5
0.25
A2G
1
1
A sample of hydrogen is mixed with air and ignited. State what would happen.
(i) The hydrogen would burn ____________ with a pop sound.
Other Answer Choices:
relight
turn red litmus blue
turn litmus white
explode
go cloudy
1
The test for chlorine is that damp litmus ________________
Other Answer Choices:
explode
turns white
turn red litmus blue
go cloudy
relight
1
The test for ammonia is that it can _________________________
Other Answer Choices:
turn red litmus blue
go cloudy
relight
explode
turns white
1
The test for CO2 is that it can make lime water ______________
Other Answer Choices:
turns white
relight
go cloudy
explode
turn red litmus blue
1
The test for O2 is that it can make a glowing splint ____________
Other Answer Choices:
go cloudy
turn red litmus blue
relight
explode
turns white
1
Graph reading
  • (ii) The volume of hydrogen produced is ___________ / twice the volume of oxygen (at each time interval).
Other Answer Choices:
triple
double
quadruple
1

Molten lead bromide is electrolysed.
The products of this electrolysis are:

2
Calcium nitrate and calcium carbonate are both ionic compounds.
Calcium nitrate mixed with water behaves as an electrolyte. Calcium carbonate mixed with water does not behave as an electrolyte.
Explain, in terms of solubility and movement of ions, this difference in behaviour.
(c) Calcium nitrate is ____________ and forms ions ________ free to move Calcium carbonate is ______________so the ions ____________ free to move in calcium carbonate (solution)
Other Answer Choices:
insoluble
soluble
are
are not
2
When molten zinc chloride is electrolysed, zinc ions, Zn^{2+}, form zinc atoms.
Write the half equation for this reaction.
Zn2++______ e−⟶Zn
Other Answer Choices:
1
3
2
1
8.000 g of CaCO3 was heated strongly for about 10 minutes. 6.213 g of solid remained.


Calculate the mass of carbon dioxide gas given off.
While this is not a mole calculation i have added in a few steps for practice.
RFM of CaCO3 = 40 + 12 + 3x 16 = ________
RFM of CaO = 40 + 16 = _______
RFM of CO2 = 12 + 2 x 16 = _______
mass of carbon dioxide = 8.000 - 6.213 __________ g
(note the question does not ask for S.f. so 1.8g and 1.79g would also score the mark.
Other Answer Choices:
100
44
56
1.787
2
The theoretical yield of calcium oxide in this experiment is 5.600 g. Calculate the percentage yield of calcium oxide.


percentage yield = ___________ mass of product / _____________ mass of product x 100
percentage yield = __________ / __________ x 100
percentage yield =_________
Other Answer Choices:
actual
97.3
expected
5.450
5.600
1

The mass of solid left in the crucible is less than the theoretical mass of calcium oxide that should be obtained. A possible reason for this is that

1

(d) (i) Calculate the relative formula mass of calcium carbonate, CaCO3. (relative atomic masses: C = 12, O = 16, Ca = 40)

1

(ii) Calculate the atom economy for the formation of calcium oxide in this reaction.
CaCO_3 \rightarrow CaO + CO_2
You must show your working. (relative atomic masses: C = 12, O = 16, Ca = 40; relative formula mass: calcium oxide = 56)

1
In the first stage of extracting nickel from nickel sulfide, the nickel sulfide, NiS, is heated in air to form nickel oxide, NiO, and sulfur dioxide.
Write the balanced equation for this reaction.
__________NiS + __________O2 -> __________NiO + __________SO2

(2)
1

An advantage of producing a metal by electrolysis is that:

7
Hydrated copper sulfate, CuSO_4.5H_2O, is a blue solid. Anhydrous copper sulfate, CuSO_4, is a white solid.
Heat energy is needed to convert hydrated copper sulfate to anhydrous copper sulfate.

This is a reversible reaction. CuSO_4.5H_2O \rightleftharpoons CuSO_4 + 5H_2O

Devise an experiment to show that this is a reversible reaction. (4)

Take hydrated copper sulfate (_________ ) place in a boiling tube.
Heat the hydrated copper sulfate with a Bunsen burner.
Observe that the colour changes from blue to __________ .
Observe that a clear ________________ liquid forms at the top of the boiling tube.
Leave the sample to cool down.
Use a dropping pipette to add a few drops of __________ to the sample.
Observe that __________ is given off and the __________ anhydrous copper sulphate is hydrated and becomes _________ hydrated copper sulfate.
Other Answer Choices:
white
colourless
blue
steam
water
3
Hydrogen reacts with iodine to form hydrogen iodide.
Iodine gas is purple and hydrogen iodide gas is colourless.
H_2(g) + I_2(g) \rightleftharpoons 2HI(g)
Hydrogen and iodine are placed in a sealed container.
The container is left until equilibrium is reached. The conditions are changed favouring the forward reaction.
Explain what you would see. (2)
The colour would become __________ as the concentration of the reactants has ______________ so there is less of the coloured ______________________ gas.
Other Answer Choices:
hydrogen
paler
iodine
darker
hydrogen iodide
decreased
1

(c) Calculate the number of atoms combined in one mole of copper iodide, CuI2.
(Avogadro constant = 6.02 \times 10^{23})
______ x 1024

1

When a metal corrodes

1

After a few days the two boiling tubes were examined. The results are shown in Figure 5.
boiling tube A: the appearance of the iron rod is unchanged
the magnesium has started to disappear
boiling tube B: a small amount of brown deposit has formed around the rod
Explain the results of this experiment.

1

Hydrazine, N_2H_4, reacts with oxygen.
N_2H_4 + O_2 \rightarrow N_2 + 2H_2O
A metal in water corrodes faster than an identical piece of metal in the same volume of water containing dissolved hydrazine. Use the information to explain how hydrazine slows corrosion.

(d) Ammonia is used to make hydrazine.
In the industrial process to manufacture ammonia, nitrogen and hydrogen are combined in the presence of an iron catalyst.
N_2 + 3H_2 \rightleftharpoons 2NH_3
1

State the name of the industrial process to manufacture ammonia.

1

Predict the effect that adding the catalyst has on the rate of attainment of equilibrium.

1

Predict the effect that adding the catalyst has on the equilibrium yield of ammonia.

Pieces of zinc react with copper sulfate solution. Zinc sulfate solution is colourless.
Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
1

Describe what you would see when an excess of zinc is added to copper sulfate solution and the mixture left until the reaction is complete. (2)

1

This reaction is described as a redox reaction.
Explain, in terms of electrons, which particles have been oxidised and which particles have been reduced in this reaction. (4)

The copper sulfate solution used has a concentration of 15.95 \, \text{g dm}^{-3}.
1

Calculate the number of moles of copper sulfate, \text{CuSO}_4, in 50.00 \, \text{cm}^3 of this solution. (relative atomic masses: \text{O} = 16, \text{S} = 32, \text{Cu} = 63.5)

1

number of moles of copper sulfate = ..................... mol

In another experiment, 0.043 \, \text{mol} of copper sulfate, \text{CuSO}_4, is used.
1

Calculate, to one decimal place, the minimum mass of zinc that must be added to react with all the copper sulfate. (relative atomic mass: \text{Zn} = 65)

1

mass = ..................... g

X and Y are solutions of two different acids. The concentration of acid in each solution, in mol dm-3, is the same. Solution X has a pH of 3.40 and solution Y has a pH of 4.40.
1

State what could be used to measure these pH values of 3.40 and 4.40.

1

What is the concentration of hydrogen ions in solution X compared with that in solution Y?

1

.....................................................................................................

1

.....................................................................................................

(b) An experiment is planned to record the change in pH as a powdered base is added to 50 \, \text{cm}^3 dilute hydrochloric acid.
The method suggested is:
  1. add dilute hydrochloric acid up to the 50 \, \text{cm}^3 mark on a beaker
  2. add one spatula of the base and stir
  3. measure the pH of the mixture
  4. repeat steps 2 and 3 until the pH stops changing.
1

(i) State how you could change the method so that the amounts of dilute hydrochloric acid and of the base can be measured more accurately. (2)
dilute hydrochloric acid .......................................................................................................................
.....................................................................................................................................................................
base ..............................................................................................................................................................
.....................................................................................................................................................................

1

(ii) During the experiment the pH changes from 2 to 10. If phenolphthalein indicator is added at the beginning of the experiment, a colour change occurs as the base is added.
State the colour change that occurs. (1)

1

colour at start ..............................................................................................................................
colour at end ................................................................................................................................

1

(iii) Explain, in terms of the particles present, why the pH increases during the experiment. (2)
.....................................................................................................................................................................
.....................................................................................................................................................................
.....................................................................................................................................................................
.....................................................................................................................................................................

Some properties of four solids, A, B, C and D, are shown in Figure 6.
The solids, in no particular order, are copper carbonate, copper oxide, magnesium metal and sodium hydroxide.
A Colour of solid: black B Colour of solid: silver C Colour of solid: white D Colour of solid: green

Observation when solid is added to water

  • A: black solid remains
  • B: a few bubbles appear on surface of solid
  • C: solid dissolves and forms colourless solution
  • D: green solid remains

pH of mixture of solid added to water

  • A: 7
  • B: 8
  • C: 13
  • D: 7

Observation when solid is added to dilute sulfuric acid

  • A: on warming, solid disappears to form blue solution
  • B: effervescence, solid disappears to form colourless solution
  • C: solid disappears to form colourless solution
  • D: effervescence, solid disappears to form blue solution
1

Identify the solids A, B, C and D, explaining how the information in Figure 6 supports the identification of each solid.
(6)

(a) Nitric acid can be titrated with a solution of ammonia.
1

State the type of reaction occurring when nitric acid reacts with ammonia.

1

What salt is formed in this reaction?

In one stage of the production of nitric acid, nitrogen oxide, NO, is reacted with oxygen to make nitrogen dioxide, NO2.
\(2NO + O_2 \rightarrow 2NO_2\)
1

Calculate the minimum volume of air, measured at room temperature and pressure, required to react with 1000 g nitrogen oxide to form nitrogen dioxide.
Assume that the air contains 20% oxygen by volume. (relative atomic masses: N = 14, O = 16) 1 mol of gas occupies 24 dm3 at room temperature and pressure)

1

Volume of air = .......... dm3

(c) In another stage in the production of nitric acid, ammonia is reacted with oxygen to form nitrogen oxide and water.
4\text{NH}_3(g) + 5\text{O}_2(g) \rightleftharpoons 4\text{NO}(g) + 6\text{H}_2\text{O}(g)
Heat energy is given out when ammonia reacts with oxygen.
The conditions chosen for the reaction are:
  • excess air, rather than just the right amount
  • a pressure of 10 atm, rather than atmospheric pressure
  • a temperature of 900 °C, rather than room temperature
1

Explain the effect of the conditions chosen on the equilibrium yield of nitrogen oxide and on the rate of attainment of equilibrium.
(6 marks)