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CHEM1832-Chemistry for Health Science (T1 2025)
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Consider the following equilibrium reaction:
H2CO3 (aq) ⇌ H+ (aq) + HCO3– (aq); K = 5.0 x 10–7
If the initial concentrations of the species are:
[H2CO3] = 0.080 M; [H+] = 1.00 x 10–5 M; [HCO3–] = 4.00 x 10–3 M
Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?
For the reaction graph below, which letter corresponds to the reaction at chemical equilibrium?
A decomposition reaction was determined to be first order.
After 842 seconds 44.8% of the starting material had been consumed.What is the half life for this reaction?
The peroxydisulfate ion (S2O82–) reacts with the iodide ion in aqueous solution via the reaction:
S2O82–(aq) + 3 I–(aq) 2 SO4(aq) + I3–(aq)
An aqueous solution containing 0.050 M of S2O82– ion and 0.072 M of I– is prepared, and the progress of the reaction followed by measuring [I–]. The data obtained is given in the following table:
| Time (s) | 0.0 | 400.0 | 800.0 | 1200.0 | 1600.0 |
| [I–] (M) | 0.072 | 0.057 | 0.046 | 0.037 | 0.029 |
The average rate of disappearance of I– in the initial 400.0 s is ________ M/s
Of the following, which are NOT valid units for a reaction rate?
Consider the reaction A + B → C. A series of reactions have been performed using different initial reactant concentrations, and the initial reaction rates have been measured:
- [A] = 5 M; [B] = 5 M; Rate = 0.4 M s-1
- [A] = 2.5 M; [B] = 5 M; Rate = 0.1 M s-1
- [A] = 2.5 M; [B] = 2.5 M; Rate = 0.05 M s-1
What is the value of the rate constant k?
The data in the table below were obtained for the reaction:
2 ClO2(aq) + 2 OH–(aq) ClO3–(aq) + ClO2–(aq) + H2O
| Experiment Number | [ClO2] (M) | [OH–] (M) | Initial Rate (M/s) |
| 1 | 0.060 | 0.030 | 0.0248 |
| 2 | 0.020 | 0.030 | 0.00276 |
| 3 | 0.020 | 0.090 | 0.00828 |
What is the order of the reaction with respect to ClO2?
Kinetic data was recorded for a chemical reaction and the graphs below were were produced using the data. Based on these graphs, determine the overall order of the rate law for this reaction.
Which of the expressions below is the integrated rate law for a zeroth order reaction?
Checkpoint #3
You should now be able to...
Calculate the half-life of a reactant in a first-order reaction.
Identify the difference between a differential and an integrated rate equation.
Apply the integrated first order rate equation.
Practice Question 1
A reaction was found to be first order with a rate constant of 4.38 × 10-4 s-1.
How much of the starting material remains after 2675 seconds?