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Learners use the reaction of MgCO₃(s) with DILUTE HCl(aq) to investigate the relationship between temperature and the rate of a chemical reaction - NSC Physical Sciences - Question 5 - 2022 - Paper 2
Question 5
Learners use the reaction of MgCO₃(s) with DILUTE HCl(aq) to investigate the relationship between temperature and the rate of a chemical reaction. The balanced equa... show full transcript
Worked Solution & Example Answer:Learners use the reaction of MgCO₃(s) with DILUTE HCl(aq) to investigate the relationship between temperature and the rate of a chemical reaction - NSC Physical Sciences - Question 5 - 2022 - Paper 2
Step 1
Step 2
Step 3
5.3 Use collision theory to explain the relationship shown in the graph.
Answer
The graph indicates that increasing temperature leads to an increased reaction rate. According to collision theory, a higher temperature means that particles have greater kinetic energy and collide more frequently, which results in a higher number of successful collisions and an increased rate of reaction.
Step 4
5.4.1 The time taken for the reaction to go to completion.
Answer
To determine the time taken for the reaction to complete, we use the average rate of reaction, which can be calculated using the formula:
ext{Rate} = rac{ ext{Change in concentration}}{ ext{Time}}
Substituting the known values, we find that the time taken is approximately 5.28 minutes.
Step 5
5.4.2 Molar gas volume at 40 °C if 1.5 dm³ CO₂ is collected.
Answer
At 40 °C, the molar volume of a gas can be calculated by:
V_m = rac{n}{V}
Where:
- n is the amount of substance in moles
- V is the volume in dm³.
Given that 1.5 dm³ of CO₂ was collected, we can rearrange the equation to calculate the molar volume, which yields 25 dm³ mol⁻¹.
Step 6
5.5 Draw the graph showing the Maxwell-Boltzmann distribution curve for CO₂(g) at 40 °C.
Answer
To illustrate the Maxwell-Boltzmann distribution curve, plot the kinetic energy on the x-axis and the number of CO₂ molecules on the y-axis. The curve should peak around the average kinetic energy, showing that most molecules have energies around this value, with fewer molecules at very low or very high energies.