Question 1
Sodium hydroxide neutralises acid.
H+ + OH- ➔ H2O
In a 11,000 dm3 sample of an aqueous solution, the concentration of acid, [H+], is 1.26 × 10-3 moldm-3.
Which mass of solid sodium hydroxide neutralises the acid?
0.0214 g
0.0504 g
236 g
554 g
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Question 2
The gas laws can be summarised in the ideal gas equation.
pV = nRT
0.960 g of oxygen gas is contained in a vessel of volume 7.00 × 10-3 m3 at a temperature of 30°C.
Assume that the gas behaves as an ideal gas.
What is the pressure in the vessel?
1.07 kPa
2.14 kPa
10.8 kPa
21.6 kPa
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Question 3
Which gas sample contains the fewest molecules?
1.00 dm3 of carbon dioxide at 27°C and 2.0 kPa
1.00 dm3 of hydrogen at 100°C and 2.0 kPa
1.00 dm3 of nitrogen at 300°C and 4.0 kPa
1.00 dm3 of oxygen at 250°C and 3.0 kPa
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Question 4
The relative atomic mass is defined as
the mass of an atom of an element relative to 1/12th the mass of a carbon-12 atom
the mass of an atom of an element relative to the mass of a hydrogen atom
the average mass of an element relative to 1/12th the mass of a carbon atom
the average mass of an atom of an element relative to 1/12th the mass of a carbon-12 atom
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Question 5
Which reaction produces the smallest atom economy of BaCl2?
BaCl2⸱2H2O ➔ BaCl2 + 2H2O
BaO + 2HCl ➔ BaCl2 + H2O
BaCO3 + 2HCl ➔ BaCl2 + CO2 + H2O
Ba + 2HCl ➔ BaCl2 + H2
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Question 6
A student mixes 100 cm3 of 0.200 mol dm-3 NaCl(aq) with 100 cm3 of 0.200 mol dm-3 Na2CO3(aq).
What is the total concentration of Na+ ions in the mixture formed?
0.100 mol dm-3
0.200 mol dm-3
0.300 mol dm-3
0.400 mol dm-3
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Question 7
Sodium reacts with water as shown below.
2Na(s) + 2H2O(l) ➔ 2NaOH(aq) + H2(g)
Which mass of sodium reacts with water to produce 960 cm3 of hydrogen gas at RTP?
0.46 g
0.92 g
1.84 g
3.68 g
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Question 8
What is the number of oxygen atoms in 88.0 g of CO2?
3.01 × 1023
1.20 × 1024
2.41 × 1024
4.82 × 1024
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Question 9
What is the empirical formula of an oxide of nitrogen that contains 26% nitrogen by mass?
NO2
N2O3
N2O5
N4O5
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Question 10
30 cm3 of xenon are mixed with 20 cm3 of fluorine. The gases react according to the following equation. Assume that the temperature and pressure remain constant.
Xe(g) + F2(g) ➔ XeF2(g)
What is the final volume of gas after the reaction is complete?
50 cm3
40 cm3
30 cm3
20 cm3
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Question 11
In a car airbag, sodium azide (NaN3) decomposes to form sodium metal and nitrogen gas.
2NaN3(s) ➔ 2Na(s) + 3N2(g)
The sodium metal then reacts with potassium nitrate to produce more nitrogen gas.
10Na(s) + 2KNO3(s) ➔ N2(g) + 5Na2O(s) + K2O(s)
If 2.00 mol of sodium azide react in this way, how many molecules of N2 will be formed?
The Avogadro constant, L = 6.022 x 1023 mol−1.
2.41 x 1024
1.93 x 1024
1.81 x 1024
9.63 x 1023
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Question 12
A 20.0 cm3 sample of a 0.400 mol dm-3 aqueous solution of a metal bromide (MBrn) reacts exactly with 160 cm3 of 0.100 mol dm-3 aqueous silver nitrate.
What is the formula of the metal bromide?
MBr
MBr2
MBr3
MBr4
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Question 13
What is the mass, in mg, of carbon formed when 3.0 × 10-3 mol of propene undergoes incomplete combustion?
2C3H6 + 3O2 ➔ 6C + 6H2O
9.0 × 10-3
3.6 × 10-2
1.08 × 102
2.16 × 102
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Question 14
The equation for the reaction between zinc and hydrochloric acid is
Zn + 2HCl ➔ ZnCl2 + H2
What is the minimum mass, in mg, of zinc (Ar = 65.4) needed to react with 50.0 cm3 of 1.68 mol dm-3 hydrochloric acid?
2.75
5.49
2.75 × 103
5.49 × 103
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Question 15
A student is provided with 5.00 cm3 of 1.00 mol dm-3 ammonia solution. The student was asked to prepare an ammonia solution with a concentration of 0.050 mol dm-3
What volume of water should the student add?
45.0 cm3
95.0 cm3
100 cm3
995 cm3
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Question 16
Nitration of 1.70 g of methyl benzoate (Mr = 136.0) produces methyl 3-nitrobenzoate (Mr = 181.0). The percentage yield is 65.0%
What mass, in g, of methyl 3-nitrobenzoate is produced?
0.830
1.10
1.47
2.26
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Question 17
In an experiment to identify a group 2 metal (X), 0.102 g of X reacts with an excess of aqueous hydrochloric acid according to the following equation.
X + 2HCl ➔ XCl2 + H2
The volume of hydrogen gas given off is 65 cm3 at 99 kPa pressure and 303 K.
The gas constant is R = 8.31 J K–1 mol–1.
Which is X?
barium
calcium
magnesium
strontium
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Question 18
When heated, a sample of potassium chlorate(V) (KClO3) produced 67.2 cm3 of oxygen, measured at 298 K and 110 kPa
2KClO3(s) ➔ 2KCl(s) + 3O2(g)
What is the amount, in moles, of potassium chlorate(V) that has decomposed?
The gas constant, R = 8.31 J K–1 mol–1.
9.95 × 10-4
1.99 × 10-3
2.99 × 10-3
4.48 × 10-3
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Question 19
Which sample, measured at room temperature and pressure, contains the greatest number of the stated particles?
1 g of hydrogen molecules
1 g of helium atoms
1 dm3 of hydrogen molecules
1 dm3 of helium atoms
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Question 20
5.0 g of an oxide of molybdenum contain 4.0 g of molybdenum.
What is the empirical formula of this oxide?
MoO2
Mo4O5
Mo2O3
Mo3O2
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Question 21
What is the percentage yield when 20 g of aluminium are produced from 50 g of aluminium oxide?
2Al2O3 ➔ 4Al + 3O2
76%
40%
33%
19%
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Question 22
What is the effect on the volume when the pressure of an ideal gas is doubled at the same time as the temperature (in K) is doubled?
halved
remains the same
doubled
quadrupled
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Question 23
The general gas equation can be used to calculate the Mr value of a gas.
For a sample of a gas of mass mg, which expression will give the value of Mr?
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