- [Instructor] Coupled reactions
use a thermodynamically favorable reaction
to drive a thermodynamically unfavorable reaction.
For example, let's look at a hypothetical reaction
where reactants A and B combine to form products C and i.
The standard change in free energy for this reaction,
delta G naught, let's say, is greater than zero.
And when delta G naught is greater than zero,
that's a thermodynamically unfavorable reaction.
And at equilibrium,
the equilibrium constant, K, is less than one.
When K is less than one,
that means there are more reactants than products
at equilibrium.
And if our goal is to make a lot of the product C,
that won't happen as long as this reaction
is thermodynamically unfavorable.
Next, let's look at another hypothetical reaction
where i reacts with D to form E and F as the products.
For this hypothetical reaction,
the standard change in free energy, delta G naught,
is much less than zero.
Since delta G naught for the second hypothetical reaction
is less than zero,
reaction two is thermodynamically favorable.
And at equilibrium,
the equilibrium constant, K, is much greater than one.
If K is much greater than one,
then we can assume that the second reaction essentially goes
to completion.
So all the i and the D will react together to form E and F.
And at equilibrium,
there are way more products than there are reactants.
Remember that our goal was to make a lot of the product C,
but we can't get that by just running the first reaction
by itself.
However, by coupling the first reaction,
which is thermodynamically unfavorable,
to the second reaction,
which is thermodynamically favorable,
we can make a significant amount of product C.
These two hypothetical reactions can be coupled together
because they share a common intermediate, i.
Even though reaction one is thermodynamically unfavorable,
even if it forms only a small amount of i,
since reaction two is thermodynamically favorable,
the i from reaction one will be used up in reaction two
to form the products for reaction two.
Removing the product i causes the equilibrium
to shift to the right in the first reaction,
therefore producing more of our desired product C.
So the thermodynamically favorable reaction
is driving the thermodynamically unfavorable reaction
to the right.
Since we are coupling these two reactions together,
if we add reaction one to reaction two,
the intermediate would cancel out.
And for the reactants,
we would get A plus B plus D;
and for the products, we would get C plus E plus F.
To find delta G naught for this overall equation,
we would need to add together delta G naught
for reaction one and delta G naught for reaction two.
So delta G naught for this overall equation
would be less than zero,
which tells us this overall equation
is thermodynamically favorable.
And the equilibrium constant is greater than one,
which means at equilibrium, we'll have a decent amount
of our desired product C.
Next, let's look at a practical example
of coupled reactions.
Let's say that our goal is to extract solid copper
from copper(I) sulfide.
The other product of this reaction is sulfur.
However, delta G naught for this reaction
is equal to positive 86.1 kilojoules per mole of reaction.
Since delta G naught is positive,
this reaction is thermodynamically unfavorable.
And at equilibrium, there'd be very little of our product,
so we wouldn't get very much copper.
The solution is to couple this first reaction
to a thermodynamically favorable reaction.
And that's the conversion of sulfur into sulfur dioxide.
So solid sulfur plus oxygen gas give sulfur dioxide,
and delta G naught for this reaction
is equal to negative 300.4 kilojoules per mole of reaction.
So adding our two reactions together,
the common intermediate, sulfur, cancels out,
and that gives us copper(I) sulfide plus oxygen
for the reactants goes to solid copper and sulfur dioxide
for the products.
And if we add the two delta G naught values together,
positive 86.1 plus negative 300.4
gives a delta G naught for this overall equation
equal to negative 214.3 kilojoules per mole of reaction.
Since delta G naught is negative,
now, this overall reaction is thermodynamically favorable
with an equilibrium constant greater than one.
Therefore, we will now produce a lot of copper.
So burning copper(I) sulfide in air gives us a feasible way
of extracting copper from copper(I) sulfide.
Coupled reactions are also very important in biochemistry.
For example, two amino acids are alanine and glycine.
And if these two amino acids come together,
they form what's called a dipeptide.
It's very important for the body
to be able to make dipeptides
because if we were to add on some more amino acids,
we would form what's called a polypeptide,
which eventually leads to the formation of a protein.
However, the formation of dipeptides
is thermodynamically unfavorable.
Therefore, the body needs a way
of making this reaction thermodynamically favorable
so the body can make proteins.
To do this, the body uses ATP,
which stands for adenosine triphosphate.
And here's the dot structure for ATP in the ionized form.
ATP is often called a high energy compound,
and the hydrolysis of ATP
is used to drive protein synthesis.
Next, let's look at the equation showing the hydrolysis
of ATP to ADP,
which is adenosine diphosphate and inorganic phosphate.
The standard change in free energy for the hydrolysis of ATP
is equal to negative 31 kilojoules per mole of reaction.
Since delta G naught is negative,
the hydrolysis of ATP is thermodynamically favorable.
Alanine and glycine combine
to form the dipeptide alanylglycine and water.
Delta G naught for the formation of this dipeptide
is equal to positive 29 kilojoules per mole of reaction.
Since delta G naught is positive,
this reaction is thermodynamically unfavorable.
With the help of an enzyme,
the unfavorable reaction is coupled
to the favorable reaction.
And if we add the two reactions together,
water would cancel out and give us alanine plus glycine
plus ATP for the reactants,
and alanylglycine and ADP and inorganic phosphate
for the products.
Adding the two values of delta G naught together,
we get delta G naught
is equal to negative two kilojoules per mole of reaction.
And since delta G naught is negative,
it's now favorable for the body
to synthesize this dipeptide.