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Worksheet: Relative Reaction Rates

Q1:

Bromide and bromate(V) ( B r O ) 3 ions react in an aqueous acid to form elemental bromine and water as the only products.

Write a balanced ionic equation for this reaction.

  • A 3 B r ( ) + B r O ( ) + 6 H ( ) 2 B r ( ) + 3 H O ( ) 3 + 2 2 a q a q a q a q l
  • B B r ( ) + 3 B r O ( ) + 1 8 H ( ) 2 B r ( ) + 9 H O ( ) 3 + 2 2 a q a q a q a q l
  • C 3 B r ( ) + 3 B r O ( ) + 1 8 H ( ) 3 B r ( ) + 9 H O ( ) 3 + 2 2 a q a q a q a q l
  • D 5 B r ( ) + B r O ( ) + 6 H ( ) 3 B r ( ) + 3 H O ( ) 3 + 2 2 a q a q a q a q l
  • E 4 B r ( ) + 2 B r O ( ) + 1 2 H ( ) 3 B r ( ) + 6 H O ( ) 3 + 2 2 a q a q a q a q l

Write the rate of reaction of bromate(V) ions in terms of the rate of reaction of bromide ions.

  • A d B r O d d B r d [ ] 𝑡 = 1 5 [ ] 𝑡 3
  • B d B r O d d B r d [ ] 𝑡 = 3 [ ] 𝑡 3
  • C d B r O d d B r d [ ] 𝑡 = 2 [ ] 𝑡 3
  • D d B r O d d B r d [ ] 𝑡 = 1 3 [ ] 𝑡 3
  • E d B r O d d B r d [ ] 𝑡 = [ ] 𝑡 3

If the rate of formation of bromine is 6 . 0 × 1 0 6 M/s, calculate the rate of reaction of bromide ions.

  • A 6 . 0 × 1 0 6 M/s
  • B 5 . 0 × 1 0 6 M/s
  • C 1 0 × 1 0 6 M/s
  • D 3 . 0 × 1 0 6 M/s
  • E 9 . 0 × 1 0 6 M/s

Q2:

In the Haber process, ammonia is produced from nitrogen and hydrogen at high temperature and pressure: Write the rate of change in the partial pressure of ammonia in terms of the rate of change in the partial pressure of hydrogen, assuming the gas volume and temperature remain constant.

  • A d N H d d H d 𝑝 ( ) 𝑡 = 1 2 𝑝 ( ) 𝑡 3 2
  • B d N H d d H d 𝑝 ( ) 𝑡 = 3 2 𝑝 ( ) 𝑡 3 2
  • C d N H d d H d 𝑝 ( ) 𝑡 = 1 2 𝑝 ( ) 𝑡 3 2
  • D d N H d d H d 𝑝 ( ) 𝑡 = 2 3 𝑝 ( ) 𝑡 3 2
  • E d N H d d H d 𝑝 ( ) 𝑡 = 2 3 𝑝 ( ) 𝑡 3 2

Q3:

The rate of a reaction doubles for every 1 0 C increase in temperature.

If the temperature increases from 2 5 C to 5 5 C by what factor does the reaction rate change?

If the temperature decreases from 95 to 2 5 C by what factor does the reaction rate change?

  • A 1 1 2 8
  • B 1 6 4
  • C 1 4 9
  • D 1 7 0
  • E 1 2 5 6

Q4:

The first step in the production of nitric acid is the reaction of ammonia with molecular oxygen. Nitric oxide ( N O ) and water are the only products.

Write a balanced chemical equation for this reaction.

  • A 3 N H ( ) + 4 O ( ) 3 N O ( ) + 6 H O ( ) 3 2 2 g g g g
  • B 2 N H ( ) + 3 O ( ) 2 N O ( ) + 4 H O ( ) 3 2 2 g g g g
  • C 6 N H ( ) + 5 O ( ) 6 N O ( ) + 4 H O ( ) 3 2 2 g g g g
  • D 4 N H ( ) + 5 O ( ) 4 N O ( ) + 6 H O ( ) 3 2 2 g g g g
  • E 8 N H ( ) + 9 O ( ) 8 N O ( ) + 1 0 H O ( ) 3 2 2 g g g g

Write the rate of change in oxygen concentration in terms of the rate of formation of nitric oxide, assuming the gas volume remains constant.

  • A d O d d N O d [ ] 𝑡 = 5 4 [ ] 𝑡 2
  • B d O d d N O d [ ] 𝑡 = 9 8 [ ] 𝑡 2
  • C d O d d N O d [ ] 𝑡 = 5 6 [ ] 𝑡 2
  • D d O d d N O d [ ] 𝑡 = 3 2 [ ] 𝑡 2
  • E d O d d N O d [ ] 𝑡 = [ ] 𝑡 2

If the rate of formation of water is 3 . 0 × 1 0 3 M/min, calculate the rate of reaction of ammonia.

  • A 4 . 0 × 1 0 3 M/min
  • B 3 . 0 × 1 0 3 M/min
  • C 2 . 0 × 1 0 3 M/min
  • D 2 . 4 × 1 0 3 M/min
  • E 4 . 5 × 1 0 3 M/min

Q5:

Carbon monoxide reacts with nitrogen dioxide to form carbon dioxide and nitric oxide:

The rate law for this reaction is rate = 𝑘 [ N O ] 2 2 and the reactants have a constant temperature and total volume.

By what factor does the rate change if the pressure of N O 2 decreases from 0.500 atm to 0.250 atm?

  • A1
  • B 1 2
  • C2
  • D 1 4
  • E4

By what factor does the rate change if the concentration of C O changes from 0.010 M to 0.030 M?

Q6:

Bromide and bromate(V) ions react in acidic aqueous solution to form elemental bromine:

The initial reaction rate of hydrogen ions is 1 . 9 0 × 1 0 5 M/s. What is the initial reaction rate of bromide ions?

  • A 1 . 1 4 × 1 0 5 M/s
  • B 0 . 9 5 × 1 0 5 M/s
  • C 2 . 2 8 × 1 0 5 M/s
  • D 1 . 5 8 × 1 0 5 M/s
  • E 3 . 1 7 × 1 0 5 M/s

Over the first 3.00 minutes of the reaction, elemental bromine is formed at an average rate of 7 . 3 3 × 1 0 5 M/s. The pH at the start of the reaction is 2.30. Calculate the pH after 3.00 minutes.

Q7:

Chlorine trifluoride is prepared by the reaction of chlorine with fluorine: Write the rate of change in the partial pressure of chlorine in terms of the rate of change in the partial pressure of fluorine, assuming the gas volume and temperature remain constant.

  • A d C l d d F d 𝑝 ( ) 𝑡 = 2 3 𝑝 ( ) 𝑡 2 2
  • B d C l d d F d 𝑝 ( ) 𝑡 = 1 3 𝑝 ( ) 𝑡 2 2
  • C d C l d d F d 𝑝 ( ) 𝑡 = 3 2 𝑝 ( ) 𝑡 2 2
  • D d C l d d F d 𝑝 ( ) 𝑡 = 1 3 𝑝 ( ) 𝑡 2 2
  • E d C l d d F d 𝑝 ( ) 𝑡 = 3 𝑝 ( ) 𝑡 2 2