5.1 Define the term rate of a reaction. 5.2 Using the experimental setup above, state the measurements that must be made to determine the rate of this reaction. 5.3 Use the collision theory to explain how the average reaction rate in Experiment I differs from the average reaction rate in Experiment II. 5.4 The average rate of the reaction in Experiment I during the first 2.5 minutes is 4.4 × 10⁻³ mol·min⁻¹. 5.5 Calculate the number of moles of At₂(CO₃)₃ that remains in the flask after 2.5 minutes. 5.6 Calculate the maximum volume of CO₂(g) that can be prepared at 25 °C in Experiment I. Take molar gas volume at 25 °C as 24 000 cm³.

Photo AI

5.1 Define the term rate of a reaction - NSC Physical Sciences - Question 5 - 2021 - Paper 2

Question 5

5.1 Define the term rate of a reaction. 5.2 Using the experimental setup above, state the measurements that must be made to determine the rate of this reaction. 5.... show full transcript

Worked Solution & Example Answer:5.1 Define the term rate of a reaction - NSC Physical Sciences - Question 5 - 2021 - Paper 2

Step 1

Define the term rate of a reaction.

96%

114 rated

Answer

The rate of a reaction refers to the change in concentration of reactants or products per unit time. It can be expressed quantitatively as the amount of substance that reacts or is produced in a given time interval, denoted by the formula: $ext{Rate} = - rac{d[ ext{Reactants}]}{dt} ext{ or } rac{d[ ext{Products}]}{dt}$

Step 2

Using the experimental setup above, state the measurements that must be made to determine the rate of this reaction.

99%

104 rated

Answer

To determine the rate of the reaction, it is essential to measure the volume of CO₂ gas produced at regular time intervals. This can involve using a gas syringe to capture and quantify the volume of CO₂ generated during the reaction.

Step 3

Use the collision theory to explain how the average reaction rate in Experiment I differs from the average reaction rate in Experiment II.

96%

101 rated

Answer

According to collision theory, the reaction rate is influenced by the frequency and effectiveness of collisions between reactant molecules. In Experiment I, a higher concentration of HCl (1.5 mol·dm⁻³) leads to more frequent collisions between reactive particles compared to Experiment II (2 mol·dm⁻³). This results in a higher average reaction rate for Experiment I, as more effective collisions occur per unit time due to the greater number of acid particles present.

Step 4

The average rate of the reaction in Experiment I during the first 2.5 minutes is 4.4 × 10⁻³ mol·min⁻¹.

98%

120 rated

Answer

To find the average rate of reaction, we can use the formula: $ext{Average rate} = rac{n}{ ext{Δ}t}$ Here,

$n$ = total moles reacted in 2.5 minutes
$ext{Δ}t = 2.5 ext{ min}$ Substituting the values, we have: $ext{Average rate} = rac{4.4 imes 10^{-3}}{2.5}$

Step 5

Calculate the number of moles of At₂(CO₃)₃ that remains in the flask after 2.5 minutes.

97%

117 rated

Answer

Using the average reaction rate previously calculated, we can determine the change in moles: $ext{Δ}n = ext{Average rate} imes ext{Δ}t = 4.4 imes 10^{-3} ext{ mol·min}^{-1} imes 2.5 ext{ min} = 1.1 imes 10^{-2} ext{ mol}$ The initial amount of At₂(CO₃)₃ is 0.016 mol, so the remaining moles after the reaction is: $ext{Remaining moles} = 0.016 - 0.011 = 0.005 ext{ mol}$

Step 6

Calculate the maximum volume of CO₂(g) that can be prepared at 25 °C in Experiment I.

97%

121 rated

Answer

Using stoichiometry, we know that 1 mole of At₂(CO₃)₃ yields 3 moles of CO₂. Given that 0.005 moles of At₂(CO₃)₃ remain: $ext{Moles of CO₂ produced} = 0.011 ext{ mol} imes 3 = 0.033 ext{ mol}$ At 25 °C and standard atmospheric conditions, the molar volume of gas is 24,000 cm³, so: $ext{Volume of CO₂} = 0.033 ext{ mol} imes 24000 ext{ cm}^3/ ext{mol} = 792 cm^3$

5.1 Define the term rate of a reaction - NSC Physical Sciences - Question 5 - 2021 - Paper 2

Worked Solution & Example Answer:5.1 Define the term rate of a reaction - NSC Physical Sciences - Question 5 - 2021 - Paper 2

Define the term rate of a reaction.

Using the experimental setup above, state the measurements that must be made to determine the rate of this reaction.

Use the collision theory to explain how the average reaction rate in Experiment I differs from the average reaction rate in Experiment II.

The average rate of the reaction in Experiment I during the first 2.5 minutes is 4.4 × 10⁻³ mol·min⁻¹.

Calculate the number of moles of At₂(CO₃)₃ that remains in the flask after 2.5 minutes.

Calculate the maximum volume of CO₂(g) that can be prepared at 25 °C in Experiment I.

Join the NSC students using SimpleStudy...