Q1.
A student investigated the rate of reaction between marble and hydrochloric acid.
The student used an excess of marble.
The reaction can be represented by this equation.
CaCO3 (s) + 2HC1 (aq)
→ CaC12 (aq) + H2O (l) + CO2 (g)
The student used the apparatus shown in the diagram.
The student measured the mass of the flask and contents every half minute for ten
minutes.
The results are shown on the graph. Use the graph to answer the questions.
(a)
Complete the graph opposite by drawing a line of best fit.
(1)
Page 1
(b)
Why did the mass of the flask and contents decrease with time?
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(1)
(c)
After how many minutes had all the acid been used up?
.............................. minutes
(1)
(d)
The student repeated the experiment at a higher temperature. All other variables
were kept the same as in the first experiment. The rate of reaction was much faster.
(i)
Draw a line on the graph to show what the results for this second experiment
might look like.
(2)
(ii)
Why does an increase in temperature increase the rate of reaction?
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(3)
(Total 8 marks)
Q2.
Hydrogen peroxide slowly decomposes into water and oxygen.
hydrogen peroxide → water + oxygen
The reaction can be speeded up by adding manganese dioxide.
(a)
(i)
What do we call a substance that speeds up a chemical reaction without
being changed itself?
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(1)
(ii)
Give two other ways of increasing the rate of this reaction.
1 ........................................................................................................................
2 ........................................................................................................................
(2)
Page 2
(b)
The diagram shows how the rate of this reaction can be measured.
As the hydrogen peroxide decomposes, the mass of the flask and its contents
decreases.
Why does this decrease in mass take place?
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(1)
(Total 4 marks)
Page 3
Q3.
Marble is a rock that contains mainly calcium carbonate. This reacts with
hydrochloric acid.
calcium carbonate + hydrochloric acid → calcium chloride + water + carbon dioxide
The rate of this reaction was followed by measuring the mass of carbon dioxide formed.
Two 10 g samples of marble, A and B, were each reacted with 50 cm3 of dilute
hydrochloric acid, at different temperatures. The mass of carbon dioxide formed in each
reaction was recorded and plotted to produce the graph below.
Each reaction stopped when no more carbon dioxide was formed.
In both experiments some marble was left unreacted when the reaction stopped.
(a)
Explain how you can tell which sample, A or B, reacted faster with the dilute
hydrochloric acid.
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(2)
Page 4
(b)
The faster rate of reaction was caused by using a higher temperature. Explain, in
terms of particles, why a higher temperature causes a faster rate of reaction.
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(3)
(Total 5 marks)
Q4.
The apparatus shown in the diagram was used to investigate the rate of reaction of
excess marble chips with dilute hydrochloric acid, HCl. Marble is calcium carbonate,
formula CaCO3. The salt formed is calcium chloride, CaCl2.
(a)
Write a balanced equation for the reaction.
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(2)
Page 5
The following results were obtained from the experiment.
Time in Reading on balance
minutes
in g
0.5
269.6
1.0
269.3
2.0
269.0
3.0
268.8
5.0
268.7
9.0
268.6
(b)
(i)
Plot the results and draw a graph on the axes below.
(3)
(ii)
Continue the graph you have drawn to show the expected reading after11
minutes.
(1)
(iii)
On the axes above, sketch a graph of the result which would be obtained if in
a similar experiment the same mass of powdered marble was used instead of
marble chips.
(2)
(Total 8 marks)
Page 6
M1.
(a)
sensible line of best fit which goes through or close to all the points except
the anomalous point
allow wobbly / short double lines
± ½ square
1
(b)
loss of gas / loss of CO2
idea of gas produced / formed
1
(c)
7
1
(d)
(i)
steeper line from around the same starting point
and left of the points
allow crosses if they are fully correct for 1 mark
1
levelling off at 99
accept short level line at 99
± ½ square
1
(ii)
any three from:
•
particles / molecules / atoms/ ions have more energy
allow given / gain / get energy
•
move faster
ignore move about more
ignore vibrate more / faster
•
collide more often
or more chance of collisions
or bump into each other more
ignore collide quicker / faster
•
collide with more force / energy
or more particles have the activation energy
or more collisions result in reaction
or more collisions are successful
3
Page 7
[8]
M2.
(a)
(i)
catalyst / enzyme
1
(ii)
any two from
do not accept increase volume of peroxide
•
heat
•
stir / shake
•
increase concentration of peroxide / catalyst
2
(b)
oxygen lost
do not allow incorrect gas
1
[4]
M3.
(a)
A faster because: the graph line steeper / the reaction had stopped earlier
accept sample B slower because: the graph line was less
steep / the reaction stopped later
A because CO2 given off faster / fizzes more for 1 mark
B because CO2 given off slower / fizzes less for 1 mark
2
(b)
increases the speed / energy of the (hydrochloric acid) particles
1
collide more frequently
1
collide more energetically / successfully
accept more successful collisions = 2 marks
1
[5]
Page 8
M4.
(a)
CaCO3 + 2HC1 → CaC12 + CO2 + H2O
one mark for CO2 and H2O or H2CO3
one mark for balancing the equation
2
(b)
(i)
linear suitable scale for y axis
± one small square
1
accurate plots
deduct one mark for each error plot
1
smooth curve through the points or a line of best fit
this mark requires a neat smooth curve
1
(ii)
curve becomes almost horizontal at or above 268.5
do not credit a straight line reaching 268.5 at 11 mins
accept a plot at 268.6
1
(iii)
steeper initial part to curve
1
becoming nearly horizontal between 268.6 and 268.4 g
1
[8]
Page 9