Topic 1 Review

What volume, in cm³, of 0.200 mol dm^–3 HCl(aq) is required to neutralize 25.0 cm³ of 0.200 mol dm^–3 Ba(OH)₂(aq)? 

• 12.5 
• 25.0 
• 50.0
• 75.0

The volume of an ideal gas at 27.0 °C is increased from 3.00 dm³ to 6.00 dm³. At what temperature, in °C, will the gas have the original pressure? 

• 13.5
• 54.0
• 327
• 600

What volume of sulfur trioxide, in cm³, can be prepared using 40 cm³ sulfur dioxide and 20 cm³ oxygen gas by the following reaction? Assume all volumes are measured at the same temperature and pressure. 
2SO₂(g) + O₂(g) → 2SO₃(g) 

• 20
• 40
• 60
• 80

Which sample has the greatest mass? 

• 6.0 x10²⁵ molecules of hydrogen 
• 5.0 mol of neon atoms 
• 1.2 x10²⁴ atoms of silver 
• 1.7 x10² g of iron 

What is the number of oxygen atoms in one mole of CuSO₄•5H₂O? 

• 5
• 9
• 6.0x10²³
• 5.4x10²⁴

What is the sum of the coefficients for the equation when balanced using the smallest possible whole numbers? 
N₂H₄(g) + O₂(g) → NO₂(g) +H₂O(g) 

• 5
• 6
• 7
• 8

What is the coefficient for H₂SO₄(aq) when the following equation is balanced, using the smallest possible integers? 
Mg₃N₂(s) + H₂SO₄(aq) → MgSO₄(aq) + (NH₄)₂SO₄(aq) 

• 1
• 3
• 4
• 7

Air bags in cars inflate when sodium azide decomposes to form sodium and nitrogen:
2NaN₃(s) → 2Na(s) + 3N₂(g)
Calculate the amount, in moles, of nitrogen gas produced by the decomposition of 2.52 mol of NaN₃(s). 

• 1.68
• 2.52
• 3.78
• 7.56

Which non-metal forms an oxide XO₂ with a relative molecular mass of 60? 

• C
• N
• Si
• S

What is the maximum mass, in g, of magnesium oxide that can be obtained from the reaction of oxygen with 2.4 g of magnesium? 

• 2.4
• 3.0
• 4.0
• 5.6