If the object on the right gained mass so that it had as much mass as the
1 answer:
You might be interested in
Answer:
The reaction isn't yet at equilibrium. The overall reaction will continue to move in the direction of the products.
Assumption: this system is currently at .
Explanation:
One way to tell whether a system is at its equilibrium is to compare its reaction quotient with the equilibrium constant
of the reaction.
The equation for is quite similar to that for
. The difference between the two is that
requires equilibrium concentrations, while
can be calculated even when the system is on its way to equilibrium.
For this reaction,
.
Given these concentrations,
.
The question states that at ,
. Assume that currently this system is also at
. (The two temperatures need to be the same since the value of
depends on the temperature.)
It turns out that . What does this mean?
- First, the system isn't at equilibrium.
- Second, if there's no external changes, the system will continue to move towards the equilibrium. Temperature might change. However, eventually
will be equal to
, and the system will achieve equilibrium.
In which direction will the system move? At this moment, . As time proceeds, the value of
will increase so that it could become equal to
. Recall that
is fraction.
When the value of increases, either its numerator becomes larger or its denominator becomes smaller, or both will happen at the same time. However,
- Concentrations on the numerator of
- Concentrations on the denominator of
As time proceeds,
- the concentration of the products will increase, while
- the concentration of the reactants will decrease.
In other words, the equilibrium will move towards the products.
Answer:
The final pressure is 0.788 atm (option b).
Explanation:
Boyle's law says that the volume occupied by a given gaseous mass at constant temperature is inversely proportional to pressure. That is: if the pressure increases, the volume decreases, while if the pressure decreases, the volume increases. This is expressed mathematically as the product of pressure times volume equal to a constant value:
P*V=k
Assuming a certain volume of gas V1 that is at a pressure P1 at the beginning of the experiment, by varying the volume of gas to a new value V2, then the pressure will change to P2, and it will be fulfilled:
P1*V1=P2*V2
In this case:
- P1= 2.14 atm
- V1= 3 L
- P2= ?
- V2= 8.15 L
Replacing:
2.14 atm*3 L= P2* 8.15 L
Solving:
0.788 atm= P2
<u><em>The final pressure is 0.788 atm (option b).</em></u>