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C1 > Chemical reactions > Flashcards

Chemical reactions Flashcards

1
Q

(3) Write the balanced equation for water decomposing to form hydrogen and
oxygen.

A 
2H2O → 2H2 + O2
• reactant formula (1)
• product formulae (1)
• balancing correct formulae
(1)
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2
Q

(2) Describe the test to show that a gas is hydrogen.

A

lighted splint
gas burns( 1)
• with (squeaky) pop (if air
present) (1)

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3
Q

(2) Describe the test to show that a gas is oxygen.

A 
glowing splint (1)
• relights (1)
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4
Q

(1) Seawater can also be decomposed using electrolysis.
Seawater is sodium chloride solution.
When this is decomposed one product is a toxic gas.
The toxic gas produced is

A

chlorine

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5
Q

(1) Give a safety precaution that should be taken when collecting this toxic gas.

A

use a fume cupboard/open all the
windows /(good) ventilation/wear a
gas mask

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6
Q

(1) When dilute hydrochloric acid reacts with copper oxide one of the products is

A

copper chloride

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7
Q

(2) Explain what is meant by electrolysis.

A 
decomposition /break
down of {compound /
substance / electrolyte}(1)
• using electricity / electrical
energy / d.c supply (1)
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8
Q

(3) Chlorine gas reacts with sodium hydroxide solution to form sodium chlorate(I), NaOCl, sodium chloride and water
Write the balanced equation for this reaction

A

reactant formulae (1)
• product formulae (1)
• balancing correct formulae
(1)

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9
Q

(1) Sodium chloride solution can be prepared by reacting sodium hydroxide solution
with an acid.
Give the name of the acid that must be used.

A

hydrochloric (acid)

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10
Q

(1) Which row of the table correctly identifies chalk, marble and limestone as
sedimentary or metamorphic rocks?

A

sedimentary / metamorphic /

sedimentary

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11
Q

(2) Suggest how you could show that, when calcium carbonate is heated, a
reaction takes place.

A 
{find mass of / weigh} solid before
heating (1)
• (heat in a suitable container) and
{find mass / weigh} again (when
cool) (1)
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12
Q

(2) Describe what you would observe when water is added, one drop at a time, to
cold calcium oxide

A 
fizzing / hissing (1)
• steam (1)
• swells (1)
• solid crumbles (to a powder) (1)
• becomes hot (1)
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13
Q

(2) Write the balanced equation for the reaction of calcium hydroxide with
carbon dioxide

A

Ca(OH)2 + CO2 → CaCO3 + H2O

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14
Q

(1) State the common name for calcium hydroxide solution.

A

limewater

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15
Q

(2) Explain why calcium carbonate removes acidic gases from emissions in power
station chimneys.

A 
(calcium carbonate) reacts with
{acidic gases / sulphur dioxide} (1)
• (because) calcium carbonate is a
base (1)
• to form a salt / calcium sulfate (1)
• neutralisation (reaction) (1)
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16
Q

(1) State a hazard associated with chlorine gas.

A

toxic / poisonous (gas)

17
Q

(2) Describe a test that can be used to identify a sample of gas as chlorine.

A

(damp blue) litmus (paper)
(1)
• (turns red then) white /
bleaches (1)

18
Q

(1) State a use of chlorine.

A 
making {poly(chloroethene / PVC /
solvents / medicines / agrochemicals /
disinfectants}
bleach / sterilising water / killing
bacteria
19
Q

(2)sodium chloride solution is electrolysed.
………….. NaCl + ………….. H2
O ……………………………… + ……………………………… + ………………………………

A

2NaCl + 2H2O → 2NaOH + H2

+ Cl2

20
Q

(6) Use these results of electrolysis to compare the volumes of hydrogen and oxygen
formed and to show the effect of changing the time and the current on the
volumes of these gases.

A

Comparing volumes of hydrogen and oxygen
• (in each experiment) volume of hydrogen is twice volume of
oxygen
• because water molecules contain twice as many hydrogen
atoms as oxygen atoms / is H2O
• overall 2H2O → 2H2 + O2
Relating volumes of gases to current and time
• (from experiments 1 and 2) time doubles
• (from experiments 1 and 2) volumes of gases double
• Volumes of gases are directly proportional to the time for
electrolysis / passage of current
• (from experiments 1 and 3) as current x 1.5
• (from experiments 1 and 3) volumes of gases x 1.5
• volumes of gases are directly proportional to the current

21
Q

(1) Sodium chloride solution can be prepared by reacting sodium hydroxide solution
with an acid.
Give the name of the acid that must be used.

A

hydrochloric (acid)

22
Q

(1) State the form of energy used to carry out the electrolysis

A

electrical (energy) / electricity /

direct (electric) current

23
Q

(1) Name the gas formed at the other electrode.

A

hydrogen

24
Q

(2) Describe the test to show that a gas is chlorine.

A

(damp blue or red) litmus (paper)

((turns red and) bleached / white

25
Q

(1) Which of these can be used to obtain chlorine from sea water?

A

electrolysis

26
Q

(1) acid + metal carbonate salt + water + ………………………………………………………………………………

A

carbon dioxide

27
Q

(2) CuO + ………….. HCl CuCl2= + ……………………….

A

CuO + 2 HCl → CuCl2 + H2O

28
Q

(1) An acid reacts with a metal oxide to form

A

a salt and water only

29
Q

(2) State two things you would see when solid copper carbonate reacts with
dilute nitric acid.

A 
(acid) colourless
(liquid/solution) (1)
• (carbonate) green (solid)
(1)
• disappears (1)
• effervesces/fizzes/bubbles
(1)
• blue (solution) (forms) (1)
30
Q

(3) Write the balanced equation for the reaction of copper carbonate with dilute nitric acid

A

CuCO3 + 2HNO3 → Cu(NO3)2 + H20 + CO2

31
Q

(2) Explain what is meant by electrolysis

A 
decomposition (of
compound/substance) (1)
M1
• (by) (direct electric)
current (1) M2
32
Q

(2) Describe a test to show the gas is oxygen.

A 
glowing splint (1) M1
• relights (1) M2
33
Q

(2) Explain what is meant by electrolysis

A

decomposition (of
compound/substance
/electrolyte)(1)
• using (direct) current (1)

34
Q

(2) Describe the test to show that a gas is chlorine.

A

(damp blue) litmus (paper)
(1)
• (turns red then) {bleaches
/ goes white} (1)

35
Q

(1) C6H9Cl3

State the name of the polymer

A

poly(chloroethene)

36
Q

(1) The reaction produces silver chloride as a precipitate.

In an equation this would be shown as

A

AgCl(s)

37
Q

(1) The total mass of this apparatus was measured.
The flask was shaken to allow the silver nitrate solution and dilute
hydrochloric acid to react.
After the reaction the total mass of the apparatus was measured again.
State how the total mass of the apparatus after the reaction will compare with
the total mass of the apparatus before the reaction.

A

same/no change

38
Q

(2) Write the balanced equation for the reaction of silver nitrate solution, AgNO3
,
with dilute hydrochloric acid to form silver chloride, AgCl, and nitric acid.

A

HCl + AgNO3 → AgCl + HNO3

39
Q

(1) Dilute sulfuric acid was added to magnesium oxide.

State the name of the salt formed.

A

magnesium sulphate

C1 (10 decks)

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