In a chemical reaction, compounds X and Y react to form a product. Let and denote the concentrations, in mol per kilolitres (mol/kL), of and respectively, at time minutes after the start of the experiment. The initial concentrations of and are given by and mol/kL.
- (a)
In a particular experiment where is present in excess, the reaction rate can be modeled as a pseudo-first-order reaction, leading to the differential equation , where is a positive constant.
- (i)
Solve this differential equation, expressing in terms of , and .
- (ii)
The half-life of the reaction, denoted by , is defined as the time taken for the concentration of to decrease to half its initial value. Show that .
- (i)
- (b)
In another experiment conducted by a chemist, the rate of the reaction is directly proportional to the product of the concentration of and the square of the concentration of . It is also known that at any instance during the reaction, every 1 mol of reacts with every 2 mol of , giving the equation .
The initial concentrations of and are 1 mol/kL and 4 mol/kL respectively.
- (i)
Show that , where is a positive constant.
- (ii)
It is given that the concentration of is 0.5 mol/kL at the instance 1 min after the start of the experiment. Find the concentration of at the instance 2 min after the start of the experiment, giving your answer to 3 significant figures.
- (i)
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Worked solution
11(a)(i)
1. Separate the variables $x$ and $t$, and set up the integrals.
2. Integrate both sides to obtain the general solution.
(Since represents concentration, and the absolute value can be omitted.)
3. Apply the initial condition to find the constant of integration.
Given that the initial concentration of is , when , .
4. Rearrange the equation to express $x$ in terms of $t$, $x_0$ and $a$.
11(a)(ii)
1. Set up the equation using the given definition of half-life and the solution from part (a)(i).
From part (a)(i), the solution to the differential equation is .
Given that is the time taken for to reach half its initial value (), substitute and into the equation:
2. Simplify and solve the resulting exponential equation for $t_{0.5}$.
Divide both sides by :
Take the natural logarithm on both sides:
t_{0.5} = \frac{\ln 2}{a} \text{ (shown)}
11(b)(i)
1. Express $y$ in terms of $x$ using the initial conditions.
Given the equation , and the initial concentrations and :
2. Formulate the differential equation and substitute $y$ to obtain the final equation.
The rate of the reaction (the rate of consumption of ) is proportional to . Since the concentration of is decreasing, its rate of change is negative:
Substituting into the equation:
Letting , which is a positive constant since , we have:
11(b)(ii)
1. Separate variables and perform partial fraction decomposition on the integrand.
Let .
Substituting gives .
Substituting gives .
Comparing coefficients of : .
Thus, .
2. Integrate both sides to obtain the general solution.
Since concentration , this simplifies to:
3. Use the initial condition $x = 1$ at $t = 0$ to find the constant of integration $C$.
From the problem context, the initial concentration of is , so when .
Substituting and :
So the equation becomes:
4. Use the condition $x = 0.5$ at $t = 1$ to determine the constant $b$.
Given when :
5. Substitute $t = 2$ and solve the resulting non-linear equation for $x$ using a graphing calculator.
Substitute and the value of :
Using a graphing calculator to solve for :
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