Rate Law worksheet - Head-Royce

Name_______________________
Rate Law Worksheet
Block_________
Ms. Glogover
1. For this reaction CH 4 + 2 O 2 → CO 2 + 2 H 2 O
the following data were obtained.
Trial Initial [CH 4 ] Initial [O 2 ] Initial Rate of
Formation of H 2 O
1 100.0 kPa 50.0 kPa 15 kPa/s
2 300.0 kPa 50.0 kPa 45 kPa/s
3 100.0 kPa 100.0 kPa 30 kPa/s
4 204.5 kPa 430.2 kPa
When
changing
ONLY...
[CH 4 ]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[O 2 ]
2. For this reaction H 2 + Cl 2 → 2 HCl
the following data were obtained.
Trial Initial [H 2 ] Initial [Cl 2 ] Initial Rate of
Formation of HCl
1 1.0 M 1.0 M 0.003 M/s
2 3.0 M 1.0 M 0.009 M/s
3 1.0 M 2.0 M 0.006 M/s
4 4.1 M 2.6 M
When
changing
ONLY...
[H 2 ]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[Cl 2 ]

3. For this reaction Ag + (aq) + Cl - (aq) → AgCl (cr)
the following data were obtained.
Trial Initial [Ag + ] Initial [Cl - ] Initial Rate of
Disappearance of Cl -
1 0.1 M 0.5 M 0.05 M/s
2 0.01 M 0.5 M 0.005 M/s
3 0.1 M 1.0 M 0.10 M/s
4 0.35 M 0.50 M
When
changing
ONLY...
[Ag + ]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[Cl – ]
4. For this reaction Na + (aq) + Cl - (aq) → NaCl (cr)
the following data were obtained.
Trial Initial [Na + ] Initial [Cl - ] Initial Rate of
Disappearance of Cl -
1 1.0 M 0.5 M 0.005 M/s
2 2.0 M 0.5 M 0.010 M/s
3 1.0 M 1.0 M 0.010 M/s
4 4.6 M 2.0 M
When
changing
ONLY...
[Na + ]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[Cl – ]

5. For this reaction A + 2 B → C + 2 D
the following data were obtained.
Trial Initial [A] Initial [B] Initial Rate of
Appearance of C
1 1.0 M 0.050 M 0.10 M/s
2 2.0 M 0.050 M 0.10 M/s
3 1.0 M 0.100 M 0.40 M/s
4 3.6 M 0.390 M
When
changing
ONLY...
[A]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[B]
6. For this reaction Q + R → Z
the following data were obtained.
Trial Initial [Q] Initial [R] Initial Rate of
Formation of Z
1 0.50 M 1.0 M 0.0030 M/s
2 0.25 M 1.0 M 0.0015 M/s
3 0.50 M 2.0 M 0.0060 M/s
4 0.00034 M 0.18 M
When
changing
ONLY...
[Q]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[R]

7. For this reaction L (aq) + M (aq) → T (ppt)
the following data were obtained.
Trial Initial [L] Initial [M] Initial Rate of
Disappearance of M
1 0.20 M 0.50 M 0.050 M/s
2 0.020 M 0.50 M 0.0050 M/s
3 0.20 M 1.5 M 0.15 M/s
4 0.35 M 0.50 M
When
changing
ONLY...
[L]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[M]
8. For this reaction E + 2 G → H + J
the following data were obtained.
Trial Initial [E] Initial [G] Initial Rate of
Disappearance of E
1 1.0 M 0.5 M 0.35 M/s
2 2.0 M 0.5 M 0.35 M/s
3 1.0 M 1.0 M 1.40 M/s
4 0.75 M 0.56 M
When
changing
ONLY...
[E]
Did rate
change?
How?
Use this data to write a rate law for the reaction.
Calculate the rate constant, k, and find the rate for trial
#4 (fill in the blank in the table).
[G]