2 End-of-chapter test
Moles and equations
Atomic masses:
H = 1; S = 32.1; Mg = 24.3; O = 16.0; C = 12.0; Ti = 47.9; Na = 23.0; Cl = 35.5; N = 14.0.
Avogadro’s number = 6.02 × 1023.
1 mol of gas molecules occupies 24.0 dm3 at room temperature and pressure, r.t.p.
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Give all answers to 3 significant figures.
a Convert the following volumes to dm3.
i 15.0 cm3
ii 1250 cm3
b What is the concentration of the following solutions?
i 0.150 mol of solute is dissolved in 200 cm3
ii 0.200 mol of solute is dissolved in 2.50 dm3
iii 0.100 mol of solute is dissolved in 300 cm3
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[3]
What is the molar mass of the following in g mol–1? Give your answers to 1 decimal place.
a S8
b MgO
c H2S
d MgSO4
e SO2
[5]
When sodium reacts with titanium chloride (TiCl4), sodium chloride (NaCl) and titanium (Ti)
are produced. Give all answers to 3 significant figures.
a Write the balanced symbol equation for the reaction.
b What mass of titanium is produced from 380 g of titanium chloride?
c What mass of titanium is produced using 46.0 g of sodium?
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[2]
Give all answers to 3 significant figures.
The reaction between NaOH and HCl can be written as:
HCl + NaOH → NaCl + H2O
In such a reaction, 15.0 cm3 of hydrochloric acid was neutralised by 20.0 cm3 of
0.0500 mol dm–3 sodium hydroxide.
a What was the volume in dm3 of:
i the acid?
ii the alkali?
b Calculate the number of moles of alkali.
c Calculate the number of moles of acid and then its concentration.
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[2]
Give all answers to 3 significant figures.
Ammonium nitrate decomposes on heating to give dinitrogen oxide and water as follows:
NH4NO3(s) → N2O(g) + 2H2O(l)
a What is the formula mass of ammonium nitrate?
b How many moles of ammonium nitrate are present in 0.800 g of the solid?
c What volume of N2O gas would be produced from this mass of ammonium nitrate?
COAS Chemistry 1 Teacher Resources
Original material © Cambridge University Press 2005, 2008
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2 End-of-chapter test
6
Give all answers to 3 significant figures.
a 1.20 dm3 of hydrogen chloride gas was dissolved in 100 cm3 of water.
i How many moles of hydrogen chloride gas are present?
ii What was the concentration of the hydrochloric acid formed?
b 25.0 cm3 of the acid was then titrated against sodium hydroxide of concentration
0.200 mol dm–3 to form NaCl and water:
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[2]
NaOH + HCl → H2O + NaCl
i How many moles of acid were used?
ii Calculate the volume of sodium hydroxide used.
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[2]
[4]
Give all answers to 3 significant figures.
4.80 dm3 of chlorine gas was reacted with sodium hydroxide solution. The reaction taking
place was as follows:
Cl2(g) + 2NaOH(aq) → NaCl(aq) + NaOCl(aq) + H2O(l)
a How many moles of Cl2 reacted?
b What mass of NaOCl was formed?
c If the concentration of the NaOH was 2.00 mol dm–3, what volume of sodium hydroxide
solution was required?
Total
COAS Chemistry 1 Teacher Resources
40
Score:
Original material © Cambridge University Press 2005, 2008
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