IGCSE Chemistry ACTUAL EXAM 2026 NEWEST UPDATE WITH COMPLETE QUESTIONS AND CORRECT DETAILED ANSWERS VERIFIED 100% GRADEDC A+

IGCSE Chemistry ACTUAL EXAM 2026 \NEWEST
UPDATE WITH COMPLETE QUESTIONS AND
CORRECT DETAILED ANSWERS \VERIFIED 100%
GRADEDC A+


Write an chemical equation for BaCl₂ (aq) + Li₂SO₄ (aq) -> BaSO₄ (s)+ 2LiCl (aq).
the reaction between barium Observe a white precipitate of barium sulfate.
chloride and lithium
sulfate (Li₂SO₄). Include state
symbols.
Also, what would you see?
Describe how you would Add nitric acid and see if carbon dioxide bubbles form
test for carbonate ions,
CO₃²⁻
Describe the test for ammonia Turns damp red litmus paper blue
gas
State the expression for % yield = (actual amount of products/theoretical amount of
calculating % yield. (Triple products) x100

science only!)
Add water to anhydrous copper(II) sulfate which will
Describe the chemical test for
water change from white to blue if water is present


What is the symbol for a
reversible reaction?
The addition of water to anhydrous copper sulfate (white) + water <-> hydrated copper
anhydrous copper sulfate sulfate (blue)

can be used to test for the
presence of water. The
reaction is reversible. What is
the word equation?
Describe the colour
change.

,Ammonia and hydrogen ammonia + hydrogen chloride <-> ammonium chloride NH₃ + HCl
chloride react together in <-> NH₄Cl
a reversible reaction to
produce a white solid. What
are the word and symbol
equations?
State two features of a 1) The rate of the forward reaction is equal to the rate of
reaction that is in dynamic the backward reaction. 2) There is no overall change
equilibrium in concentrations.
Predict what will happen to Equilibrium will move to the left because there are
the equilibrium position in fewer molecules on the left hand side
the following reaction when
the pressure is increased.
Give a reason for
your prediction: CH₄(g) +
H₂O(g) <-> CO(g)
+ 3H₂(g) ΔH = +210 kJ mol⁻1
Predict what will happen to Equilibrium will move to the right because the forward reaction is
the equilibrium position in endothermic

the following reaction when
the temperature is
increased. Give a reason for
your prediction: CH₄(g) +
H₂O(g) <-> CO(g)
+ 3H₂(g) ΔH = +210 kJ mol⁻1
Predict what will happen The rate will increase
to the rate of reaction in
the following reaction when
the temperature and
pressure is increased.
Give a reason for your
prediction: CH₄(g) +
H₂O(g) <-> CO(g) + 3H₂(g) ΔH =
+210 kJ
mol⁻1
Predict what will happen to Equilibrium will move to left the because the reaction is
the equilibrium position in exothermic

the following reaction when
the temperature is

,increased. Give a reason for
your prediction: CO(g) +
H₂O(g) <-> CO₂(g)
+ H₂(g) ΔH = -42 kJ mol⁻1

, Predict what will happen to Equilibrium will move to right the because the reaction is
the equilibrium position in exothermic

the following reaction when
the temperature is
decreased. Give a reason
for your prediction: CO(g) +
2H₂(g) <->
CH₃OH(g) ΔH = -91 kJ mol⁻1
Predict what will happen to Equilibrium will move to left the because there are
the equilibrium position in more molecules on the left hand side
the following reaction when
the pressure is decreased.
Give a reason for
your prediction: CO(g) + 2H₂(g)
<->
CH₃OH(g) ΔH = -91 kJ mol⁻1
State the raw materials used nitrogen from air and hydrogen from natural gas
in the manufacture of
ammonia

State a use for N₂ making ammonia
The following Yield would decrease and energy costs would increase
reaction is used to
manufacture ammonia
in the Haber
process: N₂ + 3H₂ -> 2NH₃ ΔH
= -92KJ/mol.
The reaction is carried out at
450⁰C but the reaction would
be faster if a higher
temperature were used.
Suggest why a higher
temperature is not used in the
Haber process
State the temperature 450°C
used for the manufacture of
ammonia by the Haber
process