Non-Ideal Gas Behavior - AP Chemistry
Card 0 of 8
One flask is at STP and another is at
. What is the pressure at
?
One flask is at STP and another is at . What is the pressure at
?
The pressure of the flask at
is
.

Because the volume between the flasks and the moles in each flask are constant, we can cancel out
and
.

At STP, conditions are
and
.


The pressure of the flask at is
.
Because the volume between the flasks and the moles in each flask are constant, we can cancel out and
.
At STP, conditions are and
.
Compare your answer with the correct one above
A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.


A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.
Recall the van der Waals equation for non-ideal gases

Rewrite the equation using the known values and solve for P
![[\textrm{P + }\frac{(1\textrm{ mol})^{2}(6.49\frac{\textrm{L}^{2}\textrm{ atm}}{\textrm{mol}^{2}})}{(3.00\textrm{ L})^2}][\textrm{3.00 L - (1 mol)}(0.0562\frac{\textrm{L}}{\textrm{mol}})]=(1\textrm{ mol})^{2}(0.0821\frac{\textrm{atm}}{\textrm{mol K}})(273K)](https://vt-vtwa-assets.varsitytutors.com/vt-vtwa/uploads/formula_image/image/996927/gif.latex)


Recall the van der Waals equation for non-ideal gases
Rewrite the equation using the known values and solve for P
Compare your answer with the correct one above
One flask is at STP and another is at
. What is the pressure at
?
One flask is at STP and another is at . What is the pressure at
?
The pressure of the flask at
is
.

Because the volume between the flasks and the moles in each flask are constant, we can cancel out
and
.

At STP, conditions are
and
.


The pressure of the flask at is
.
Because the volume between the flasks and the moles in each flask are constant, we can cancel out and
.
At STP, conditions are and
.
Compare your answer with the correct one above
A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.


A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.
Recall the van der Waals equation for non-ideal gases

Rewrite the equation using the known values and solve for P
![[\textrm{P + }\frac{(1\textrm{ mol})^{2}(6.49\frac{\textrm{L}^{2}\textrm{ atm}}{\textrm{mol}^{2}})}{(3.00\textrm{ L})^2}][\textrm{3.00 L - (1 mol)}(0.0562\frac{\textrm{L}}{\textrm{mol}})]=(1\textrm{ mol})^{2}(0.0821\frac{\textrm{atm}}{\textrm{mol K}})(273K)](https://vt-vtwa-assets.varsitytutors.com/vt-vtwa/uploads/formula_image/image/996927/gif.latex)


Recall the van der Waals equation for non-ideal gases
Rewrite the equation using the known values and solve for P
Compare your answer with the correct one above
One flask is at STP and another is at
. What is the pressure at
?
One flask is at STP and another is at . What is the pressure at
?
The pressure of the flask at
is
.

Because the volume between the flasks and the moles in each flask are constant, we can cancel out
and
.

At STP, conditions are
and
.


The pressure of the flask at is
.
Because the volume between the flasks and the moles in each flask are constant, we can cancel out and
.
At STP, conditions are and
.
Compare your answer with the correct one above
A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.


A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.
Recall the van der Waals equation for non-ideal gases

Rewrite the equation using the known values and solve for P
![[\textrm{P + }\frac{(1\textrm{ mol})^{2}(6.49\frac{\textrm{L}^{2}\textrm{ atm}}{\textrm{mol}^{2}})}{(3.00\textrm{ L})^2}][\textrm{3.00 L - (1 mol)}(0.0562\frac{\textrm{L}}{\textrm{mol}})]=(1\textrm{ mol})^{2}(0.0821\frac{\textrm{atm}}{\textrm{mol K}})(273K)](https://vt-vtwa-assets.varsitytutors.com/vt-vtwa/uploads/formula_image/image/996927/gif.latex)


Recall the van der Waals equation for non-ideal gases
Rewrite the equation using the known values and solve for P
Compare your answer with the correct one above
One flask is at STP and another is at
. What is the pressure at
?
One flask is at STP and another is at . What is the pressure at
?
The pressure of the flask at
is
.

Because the volume between the flasks and the moles in each flask are constant, we can cancel out
and
.

At STP, conditions are
and
.


The pressure of the flask at is
.
Because the volume between the flasks and the moles in each flask are constant, we can cancel out and
.
At STP, conditions are and
.
Compare your answer with the correct one above
A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.


A 3.00 L container at 273 K is filled with 1.00 mol Cl2(g), which behaves non-ideally.
Using the van der Waals equation, calculate pressure exerted by the gas.
Recall the van der Waals equation for non-ideal gases

Rewrite the equation using the known values and solve for P
![[\textrm{P + }\frac{(1\textrm{ mol})^{2}(6.49\frac{\textrm{L}^{2}\textrm{ atm}}{\textrm{mol}^{2}})}{(3.00\textrm{ L})^2}][\textrm{3.00 L - (1 mol)}(0.0562\frac{\textrm{L}}{\textrm{mol}})]=(1\textrm{ mol})^{2}(0.0821\frac{\textrm{atm}}{\textrm{mol K}})(273K)](https://vt-vtwa-assets.varsitytutors.com/vt-vtwa/uploads/formula_image/image/996927/gif.latex)


Recall the van der Waals equation for non-ideal gases
Rewrite the equation using the known values and solve for P
Compare your answer with the correct one above